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Backer #2

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how different weather change

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Kids learn about temperature in the science of physics and the scales Celsius, Fahrenheit, and Kelvin. How to convert between temperature scales and about absolute zero.

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jacques picture

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How does different aspects of a substance (such as mass, type of matter) effect the amount of energy transferred

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How does different aspects of a substance (such as mass, type of matter) effect the amount of energy transferred

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How does different aspects of a substance (such as mass, type of matter) effect the amount of energy transferred

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3 States of Matter for Kids (Solid, Liquid, Gas): Science for Children - FreeSchool

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How does different aspects of a substance (such as mass, type of matter) effect the amount of energy transferred

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How does different aspects of a substance (such as mass, type of matter) effect the amount of energy transferred

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How does different aspects of a substance (such as mass, type of matter) effect the amount of energy transferred

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What Is Matter? - The Dr. Binocs Show | Best Learning Videos For Kids | Peekaboo Kidz

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Learning Objectives

By the end of this section, you will be able to:

Observe heat transfer and change in temperature and mass.

Calculate final temperature after heat transfer between two objects.

One of the major effects of heat transfer is temperature change: heating increases the temperature while cooling decreases it. We assume that there is no phase change and that no work is done on or by the system. Experiments show that the transferred heat depends on three factors-the change in temperature, the mass of the system, and the substance and phase of the substance.

The dependence on temperature change and mass are easily understood. Owing to the fact that the (average) kinetic energy of an atom or molecule is proportional to the absolute temperature, the internal energy of a system is proportional to the absolute temperature and the number of atoms or molecules. Owing to the fact that the transferred heat is equal to the change in the internal energy, the heat is proportional to the mass of the substance and the temperature change. The transferred heat also depends on the substance so that, for example, the heat necessary to raise the temperature is less for alcohol than for water. For the same substance, the transferred heat also depends on the phase (gas, liquid, or solid).

Heat Transfer and Temperature Change

The quantitative relationship between heat transfer and temperature change contains all three factors: Q = mcΔ T, where Q is the symbol for heat transfer, m is the mass of the substance, and Δ T is the change in temperature. The symbol c stands for specific heat and depends on the material and phase. The specific heat is the amount of heat necessary to change the temperature of 1.00 kg of mass by 1.00ºC. The specific heat c is a property of the substance; its SI unit is J/(kg ⋅ K) or J/(kg ⋅ ºC). Recall that the temperature change (Δ T) is the same in units of kelvin and degrees Celsius. If heat transfer is measured in kilocalories, then the unit of specific heat is kcal/(kg ⋅ ºC).

Values of specific heat must generally be looked up in tables, because there is no simple way to calculate them. In general, the specific heat also depends on the temperature. Table 1 lists representative values of specific heat for various substances. Except for gases, the temperature and volume dependence of the specific heat of most substances is weak. We see from this table that the specific heat of water is five times that of glass and ten times that of iron, which means that it takes five times as much heat to raise the temperature of water the same amount as for glass and ten times as much heat to raise the temperature of water as for iron. In fact, water has one of the largest specific heats of any material, which is important for sustaining life on Earth.

Example 1. Calculating the Required Heat: Heating Water in an Aluminum Pan

A 0.500 kg aluminum pan on a stove is used to heat 0.250 liters of water from 20.0ºC to 80.0ºC. (a) How much heat is required? What percentage of the heat is used to raise the temperature of (b) the pan and (c) the water?

Strategy

The pan and the water are always at the same temperature. When you put the pan on the stove, the temperature of the water and the pan is increased by the same amount. We use the equation for the heat transfer for the given temperature change and mass of water and aluminum. The specific heat values for water and aluminum are given in Table 1.

Solution

Because water is in thermal contact with the aluminum, the pan and the water are at the same temperature.

Calculate the temperature difference:

Calculate the mass of water. Because the density of water is 1000 kg/m ³, one liter of water has a mass of 1 kg, and the mass of 0.250 liters of water is m = 0.250 kg.

Calculate the heat transferred to the water. Use the specific heat of water in Table 1:

Calculate the heat transferred to the aluminum. Use the specific heat for aluminum in Table 1:

Compare the percentage of heat going into the pan versus that going into the water. First, find the total transferred heat:

Thus, the amount of heat going into heating the pan is

[latex]\frac{27.0\text{ kJ}}{89.8\text{ kJ}}\times100\%=30.1\%\\[/latex]

and the amount going into heating the water is

[latex]\frac{62.8\text{ kJ}}{89.8\text{ kJ}}\times100\%=69.9\%\\[/latex].

Discussion

In this example, the heat transferred to the container is a significant fraction of the total transferred heat. Although the mass of the pan is twice that of the water, the specific heat of water is over four times greater than that of aluminum. Therefore, it takes a bit more than twice the heat to achieve the given temperature change for the water as compared to the aluminum pan.

Example 2. Calculating the Temperature Increase from the Work Done on a Substance: Truck Brakes Overheat on Downhill Runs

Truck brakes used to control speed on a downhill run do work, converting gravitational potential energy into increased internal energy (higher temperature) of the brake material. This conversion prevents the gravitational potential energy from being converted into kinetic energy of the truck. The problem is that the mass of the truck is large compared with that of the brake material absorbing the energy, and the temperature increase may occur too fast for sufficient heat to transfer from the brakes to the environment.

Calculate the temperature increase of 100 kg of brake material with an average specific heat of 800 J/kg ⋅ ºC if the material retains 10% of the energy from a 10,000-kg truck descending 75.0 m (in vertical displacement) at a constant speed.

Strategy

If the brakes are not applied, gravitational potential energy is converted into kinetic energy. When brakes are applied, gravitational potential energy is converted into internal energy of the brake material. We first calculate the gravitational potential energy ( Mgh) that the entire truck loses in its descent and then find the temperature increase produced in the brake material alone.

Solution

1. Calculate the change in gravitational potential energy as the truck goes downhill Mgh = (10,000 kg)(9.80 m/s²)(75.0 m) = 7.35 × 10⁶ J.

2. Calculate the temperature from the heat transferred using Q = Mgh and [latex]\Delta{T}=\frac{Q}{mc}\\[/latex], where m is the mass of the brake material. Insert the values m = 100 kg and c = 800 J/kg ⋅ ºC to find [latex]\Delta{T}=\frac{\left(7.35\times10^6\text{ J}\right)}{\left(100\text{ kg}\right)\left(800\text{ J/kg}^{\circ}\text{C}\right)}=92^{\circ}C\\[/latex].

Discussion

This temperature is close to the boiling point of water. If the truck had been traveling for some time, then just before the descent, the brake temperature would likely be higher than the ambient temperature. The temperature increase in the descent would likely raise the temperature of the brake material above the boiling point of water, so this technique is not practical. However, the same idea underlies the recent hybrid technology of cars, where mechanical energy (gravitational potential energy) is converted by the brakes into electrical energy (battery).

Note that Example 2 is an illustration of the mechanical equivalent of heat. Alternatively, the temperature increase could be produced by a blow torch instead of mechanically.

Example 3. Calculating the Final Temperature When Heat Is Transferred Between Two Bodies: Pouring Cold Water in a Hot Pan

Suppose you pour 0.250 kg of 20.0ºC water (about a cup) into a 0.500-kg aluminum pan off the stove with a temperature of 150ºC. Assume that the pan is placed on an insulated pad and that a negligible amount of water boils off. What is the temperature when the water and pan reach thermal equilibrium a short time later?

Strategy

The pan is placed on an insulated pad so that little heat transfer occurs with the surroundings. Originally the pan and water are not in thermal equilibrium: the pan is at a higher temperature than the water. Heat transfer then restores thermal equilibrium once the water and pan are in contact. Because heat transfer between the pan and water takes place rapidly, the mass of evaporated water is negligible and the magnitude of the heat lost by the pan is equal to the heat gained by the water. The exchange of heat stops once a thermal equilibrium between the pan and the water is achieved. The heat exchange can be written as | Q hot|= Q cold.

Solution

Use the equation for heat transfer Q = mcΔ T to express the heat lost by the aluminum pan in terms of the mass of the pan, the specific heat of aluminum, the initial temperature of the pan, and the final temperature: Q hot = m Al c Al( T f − 150ºC).

Express the heat gained by the water in terms of the mass of the water, the specific heat of water, the initial temperature of the water and the final temperature: Q cold = m W c W( T f − 20.0ºC).

Note that Q hot<0 and Q cold>0 and that they must sum to zero because the heat lost by the hot pan must be the same as the heat gained by the cold water:

[latex]\begin{array}{lll}Q_{\text{cold}}+Q_{\text{hot}}&=&0\\Q_{\text{cold}}&=&-Q_{\text{hot}}\\m_{\text{W}}c_{\text{W}}\left(T_{\text{f}}-20.0^{\circ}\text{C}\right)&=&-m_{\text{Al}}c_{\text{Al}}\left(T_{\text{f}}-150^{\circ}\text{C}\right)\end{array}\\[/latex]

This an equation for the unknown final temperature, T f.

Bring all terms involving T f on the left hand side and all other terms on the right hand side. Solve for T f,

[latex]\displaystyle{T_{\text{f}}}=\frac{m_{\text{Al}}c_{\text{Al}}\left(T_{\text{f}}-150^{\circ}\text{C}\right)+m_{\text{W}}c_{\text{W}}\left(T_{\text{f}}-20.0^{\circ}\text{C}\right)}{m_{\text{Al}}c_{\text{Al}}+m_{\text{W}}c_{\text{W}}}\\[/latex],

and insert the numerical values:

[latex]\begin{array}{lll}T_{\text{f}}&=&\frac{\left(0.500\text{ kg}\right)\left(900\text{ J/kg}^{\circ}\text{C}\right)\left(150^{\circ}\text{C}\right)+\left(0.250\text{ kg}\right)\left(4186\text{ J/kg}^{\circ}\text{C}\right)\left(20.0^{\circ}\text{C}\right)}{\left(0.500\text{ kg}\right)\left(900\text{ J/kg}^{\circ}\text{C}\right)+\left(0.250\text{ kg}\right)\left(4186\text{ J/kg}^{\circ}\text{C}\right)}\\\text{ }&=&\frac{88430\text{ J}}{1496.5\text{ J}/^{\circ}\text{C}}\\\text{ }&=&59.1^{\circ}\text{C}\end{array}\\[/latex]
Discussion
This is a typical calorimetry problem-two bodies at different temperatures are brought in contact with each other and exchange heat until a common temperature is reached. Why is the final temperature so much closer to 20.0ºC than 150ºC? The reason is that water has a greater specific heat than most common substances and thus undergoes a small temperature change for a given heat transfer. A large body of water, such as a lake, requires a large amount of heat to increase its temperature appreciably. This explains why the temperature of a lake stays relatively constant during a day even when the temperature change of the air is large. However, the water temperature does change over longer times (e.g., summer to winter).

Take-Home Experiment: Temperature Change of Land and Water

What heats faster, land or water?

To study differences in heat capacity:

Place equal masses of dry sand (or soil) and water at the same temperature into two small jars. (The average density of soil or sand is about 1.6 times that of water, so you can achieve approximately equal masses by using 50% more water by volume.)

Heat both (using an oven or a heat lamp) for the same amount of time.

Record the final temperature of the two masses.

Now bring both jars to the same temperature by heating for a longer period of time.

Remove the jars from the heat source and measure their temperature every 5 minutes for about 30 minutes.

Which sample cools off the fastest? This activity replicates the phenomena responsible for land breezes and sea breezes.

Check Your Understanding

If 25 kJ is necessary to raise the temperature of a block from 25ºC to 30ºC, how much heat is necessary to heat the block from 45ºC to 50ºC?

Solution

The heat transfer depends only on the temperature difference. Since the temperature differences are the same in both cases, the same 25 kJ is necessary in the second case.

Section Summary

The transfer of heat Q that leads to a change ΔT in the temperature of a body with mass m is Q = mcΔT, where c is the specific heat of the material. This relationship can also be considered as the definition of specific heat.

Conceptual Questions

1. What three factors affect the heat transfer that is necessary to change an object's temperature?

2. The brakes in a car increase in temperature by ΔT when bringing the car to rest from a speed v. How much greater would ΔT be if the car initially had twice the speed? You may assume the car to stop sufficiently fast so that no heat transfers out of the brakes.

Problems & Exercises

1. On a hot day, the temperature of an 80,000-L swimming pool increases by 1.50ºC. What is the net heat transfer during this heating? Ignore any complications, such as loss of water by evaporation.

2. Show that 1 cal/g · ºC =1 kcal/kg · ºC.

3. To sterilize a 50.0-g glass baby bottle, we must raise its temperature from 22.0ºC to 95.0ºC. How much heat transfer is required?

4. The same heat transfer into identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.00 kcal of heat transfers into 1.00 kg of the following, originally at 20.0ºC: (a) water; (b) concrete; (c) steel; and (d) mercury.

5. Rubbing your hands together warms them by converting work into thermal energy. If a woman rubs her hands back and forth for a total of 20 rubs, at a distance of 7.50 cm per rub, and with an average frictional force of 40.0 N, what is the temperature increase? The mass of tissues warmed is only 0.100 kg, mostly in the palms and fingers.

6. A 0.250-kg block of a pure material is heated from 20.0ºC to 65.0ºC by the addition of 4.35 kJ of energy. Calculate its specific heat and identify the substance of which it is most likely composed.

7. Suppose identical amounts of heat transfer into different masses of copper and water, causing identical changes in temperature. What is the ratio of the mass of copper to water?

8. (a) The number of kilocalories in food is determined by calorimetry techniques in which the food is burned and the amount of heat transfer is measured. How many kilocalories per gram are there in a 5.00-g peanut if the energy from burning it is transferred to 0.500 kg of water held in a 0.100-kg aluminum cup, causing a 54.9ºC temperature increase? (b) Compare your answer to labeling information found on a package of peanuts and comment on whether the values are consistent.

9. Following vigorous exercise, the body temperature of an 80.0-kg person is 40.0ºC. At what rate in watts must the person transfer thermal energy to reduce the the body temperature to 37.0ºC in 30.0 min, assuming the body continues to produce energy at the rate of 150 W? 1 watt = 1 joule/second or 1 W = 1 J/s.

10. Even when shut down after a period of normal use, a large commercial nuclear reactor transfers thermal energy at the rate of 150 MW by the radioactive decay of fission products. This heat transfer causes a rapid increase in temperature if the cooling system fails (1 watt = 1 joule/second or 1 W = 1 J/s and 1 MW = 1 megawatt). (a) Calculate the rate of temperature increase in degrees Celsius per second (ºC/s) if the mass of the reactor core is 1.60 × 10⁵ kg and it has an average specific heat of 0.3349 kJ/kg ⋅ ºC. (b) How long would it take to obtain a temperature increase of 2000ºC, which could cause some metals holding the radioactive materials to melt? (The initial rate of temperature increase would be greater than that calculated here because the heat transfer is concentrated in a smaller mass. Later, however, the temperature increase would slow down because the 5 × 10⁵-kg steel containment vessel would also begin to heat up.)

Glossary

specific heat: the amount of heat necessary to change the temperature of 1.00 kg of a substance by 1.00 ºC

Selected Solutions to Problems & Exercises

1. 5.02 × 10 ⁸ J

3. 3.07 × 10 ³ J

5. 0.171ºC

7. 10.8

9. 617 W

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By the end of this section, you will be able to: Observe heat transfer and change in temperature and mass. Calculate final temperature after heat transfer between two objects. One of the major effects of heat transfer is temperature change: heating increases the temperature while cooling decreases it.

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Are you confused about the difference between chemical changes and physical changes and how to tell them apart? In a nutshell, a chemical change produces a new substance, while a physical change does not. A material may change shapes or forms while undergoing a physical change, but no chemical reactions occur, and no new compounds are produced.

There are also other indications of chemical and physical changes, such as odor and sound. Here is a look at how to recognize the two types of changes, along with telltale indications and common examples of each.

Key Takeaways

Examples of Chemical Changes

A new compound (product) results from a chemical change as the atoms rearrange themselves to form new chemical bonds. A chemical change always involves a chemical reaction. The starting materials and final product are chemically different from one another. Here are some examples of chemical changes:

Burning wood

Souring milk

Mixing acid and a base

Digesting food

Cooking an egg

Heating sugar to form caramel

Baking a cake

Rusting of iron

Examples of Physical Changes

No new chemical species forms in a physical change. Changing the state of a pure substance between the solid, liquid, or gas phase is a physical change since the identity of the matter does not change. A physical change involves changes in physical properties, but not chemical properties. For example, physical properties change during tempering steel, crystallization, and melting. Here are examples of physical changes:

Crumpling a sheet of aluminum foil

Melting an ice cube

Casting silver in a mold

Breaking a bottle

Boiling water

Evaporating alcohol

Shredding paper

Sublimation of dry ice into carbon dioxide vapor

Carbon changing from graphite into a diamond

How to Tell Physical and Chemical Changes Apart

Look for an indication that a chemical change occurred. Signs of a chemical change include the following:

Gas is produced. In liquids, bubbles may form.

An odor is produced.

The substance changes color.

Sound is produced.

There is a temperature change. The surroundings become either hot or cold.

Light is produced.

A precipitate forms.

The change is difficult or possible to reverse.

A chemical change might not display all of these signs. If you don't see any of these indications, a physical change likely occurred. Be aware a physical change may produce a dramatic change in the appearance of a substance. This doesn't mean a chemical reaction occurred. The only way to know for certain whether a change is chemical or physical is a chemical analysis of the starting and ending materials.

In some cases, it may be hard to tell whether a chemical or physical change occurred. For example, when you dissolve sugar in water, a physical change occurs. The form of the sugar changes, but it remains the same chemically (sucrose molecules). However, when you dissolve salt in water, the salt dissociates into its ions (from NaCl into Na⁺ and Cl⁻), so a chemical change occurs. In both cases, a white solid dissolves into a clear liquid, and in both cases, you can recover the starting material by removing the water, yet the processes are not the same.

Explore chemical and physical changes in greater detail. Learn how they relate to the chemical and physical properties of matter with these additional resources.

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What Are Examples of Chemical and Physical Changes?

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Here are some examples of physical changes and chemical changes, along with an explanation of how you can tell the two apart.

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Physical and Chemical Weathering of Rocks

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Elements, atoms and compounds are often too small for you to see individually. So how can you know if a chemical change has occurred? Luckily, you often don't need any sort of microscope; there are plenty of chemical changes that you can see. Let's take a look at some of the ways you can identify the evidence of a chemical change.

A chemical reaction takes place when one or more substances are changed into a new substance. This means that the chemical composition of a substance changes. It is important to remember that matter is neither created nor destroyed in a chemical reaction. Instead, a substance is simply rearranged to form another one. This new substance can be in any state of matter. Here are the five signs of chemical change.

You've probably seen this kind of chemical change before if you have left your shiny blue bike outside over the rainy winter for too long. You saw rust, of course. Rust forms on your bike when the iron in the metal frame reacts with the oxygen and water in the air. It forms a new compound called iron oxide. This change in color, from blue to reddish brown, indicates that a chemical change has taken place.

When energy is either absorbed or released, it is indicative of a chemical change. Fireworks are an example of a chemical change that produces a temperature change and emits light. Fireworks contain fuel and an oxidizing agent. As the oxidizer breaks down the fuel, it releases an enormous amount of energy. Some of this energy is released as heat, so remember to not get too close!

When two salts are mixed, it is possible for a solid substance to form and precipitate out of solution. This means that if you start with two liquids and then see a solid substance in your beaker, it is clear evidence of a chemical change.

Precipitation reactions are very important in making sure water is safe for human consumption. Water purification facilities make use of the fact that they can add a chemical to the water which will react with an impurity in the water and precipitate. Then the now-pure water can be removed from the solid which contains the impurities.

Production of gas is a clear sign that a chemical change has occurred. A quite delicious example of that is baking a cake. When you bite into a moist cake and see the tiny holes in the cake, this is indicative of the rising agent (either baking soda or baking powder) reacting with the acidic components of the cake to create carbon dioxide. This gas is what helps a cake rise in the oven.

Given this information, would water boiling be an example of a chemical change?

You may be tempted to say, "Well, I see bubbles! That means there is a chemical change." It is important to keep in mind that even though the phase of the water has changed, the chemical structure has not, and you have not made a new compound or destroyed a compound, which is important when it comes to evidence of a chemical change. Instead, this kind of change is called a physical change.

Make sure you keep in mind what a chemical change really is when looking at different chemical states.

Is the light bulb going on by now? There are many reactions that produce light and allow you to see that a chemical reaction has taken place. One example that you may have even witnessed firsthand is the reaction in a light stick. When you bend the light stick and break the small glass vial on the inside you initiate a reaction between hydrogen peroxide and phenyl oxalate ester, which results in the emission of light.

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5 Ways to Know if a Chemical Change Has Occurred

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A chemical reaction occurs when a substance is rearranged to form a new substance. It is possible to identify if this has taken place from one of the five signs of chemical change. These changes include color change, temperature change, precipitate formation, gas production and light emission.

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What Is a Chemical Change?

Have you ever looked into the sky and seen a beautiful set of fireworks on display? As amazing as fireworks are, we can also classify them as a type of chemical change. A series of chemical changes take place to produce those awesome fireworks we see.

By definition, a chemical change happens when the molecular identity of matter changes to an entirely new form. This change is irreversible; that is, there's no going back once a chemical change occurs. One way to remember this definition is to think of the term, a chemical reaction. That's right! This term should pop into your mind as a chemical change can also be called a chemical reaction.

Signs and Evidence

There are a variety of signs that may provide clues that a chemical change has entered the building. Let's look at the following five signs:

Odor

Have you ever witnessed the awful sight and smell of spoiled food? Before going bad, a chemical change must take place. The evidence of the chemical change in our food is the offensive smell. Not all the smells are bad however; the delicious smell of baking bread is due to chemical change as well.

Energy Change (Temperature and Light)

Remember that chemical changes tell you a chemical reaction is taking place. During chemical reactions, bonds that hold atoms together are constantly broken and formed, requiring or releasing energy. This energy directly affects temperature. For example, if we grab our flask and conduct a reaction where bonds are broken, we will see that a lot of energy is needed to break those bonds. By absorbing energy, don't be alarmed if the flask feels cold during the reaction.

When energy is released, it can sometimes be in the form of light, like in the glow emitted after you break a glow stick. When you're bending it, you're breaking a little tube inside that releases a liquid into the outer tube. The mix of chemicals together causes a chemical reaction that releases light as a byproduct.

Gas Bubbles

When a chemical reaction produces a gaseous product, this is an indication that a chemical change is occurring. Visually, this gaseous product is simply the presence of bubbles. This reaction can occur between two liquid solutions or even a solid added to a liquid solution. A great example can be the mixture of baking soda, a solid, with vinegar, a liquid. When you mix the two substances together, a chemical change occurs, and you can tell based on the appearance of lots and lots of bubbles.

Formation of a Precipitate

A precipitate is a fancy term for a solid substance. If you ever mix two solutions together and see a solid substance form in the container, that is a precipitate. This gives you evidence that a chemical change is taking place. When you mix potassium iodide with lead (II) nitrate you produce a beautiful yellow precipitate called lead (II) iodide.

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chemical change: signs & evidence - video & lesson transcript | study.com

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Chemical Change: Signs & Evidence - Video & Lesson Transcript | Study.com

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Have you ever looked into the sky and seen a beautiful set of fireworks on display? As amazing as fireworks are, we can also classify them as a type of chemical change. A series of chemical changes take place to produce those awesome fireworks we see.

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B.

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my answer is A

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false because the larger ice cube is bigger than the smaller ice cubes in the the larger ice cube will not have that much space for the surface.

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The zinc have different color then all of the other ones and a chemical reaction does occurs.

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particle model x: 23 C
particle model z:0 C
Particle model y: 5 and 7 C

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The answer is false because the larger ice cube is bigger than the smaller ice cubes in the the larger ice cube will not have that much space for the surface.

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Particle Model X: 23 C
Particle Model Z: 0 C
Particle Model Y: 5 and 7 C

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particle model x: 23 C
particle model z:0 C
Particle model y: 5 and 7 C

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The smaller ice cubes melt faster because they are split apart they turn into a liquid. that's why the smaller ice cubes melt faster.

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devin answer particle model x: 23 Cparticle model z:0 CParticle model y: 5 and 7 C

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devin answer particle model x: 23 Cparticle model z:0 CParticle model y: 5 and 7 C

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medium pressure 60 C
high pressure 120 C
low pressure turned off

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particle x is 23 c gas
particle y is 5 c and 7 c liquid
particle z is 0 c solid

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 devin answer Medium pressure :  hot plate set to 60 Chigh pressure : hot plate set to  120 CLow pressure  : hot plate offfavorite border

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 devin answer Medium pressure :  hot plate set to 60 Chigh pressure : hot plate set to  120 CLow pressure  : hot plate offfavorite border

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B

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devin answer

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My answer is D because if u have a larger piece of ice the liquid will have less thermal energy .

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zinc does occur

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Z solid X gas Y liquid

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Beaker #2

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False because the big ice cube can fit in the bath because of it size.
The small ice cube can because its small enough for the small ice cube to fit.

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Video

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Low pressure is Hot plate off
High pressure is Hot plate set at 120.
Medium is Hot plate set at 60.

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hot plate of is low pressure and hot plate set to 60C is medium pressure and hot plate set to 120C is high pressure

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particle x

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B

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Low Pressure - Plate off

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particle model x: 23 C
particle model z:0 C
Particle model y: 5 and 7 C

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B.

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B.

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x

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hot plate off is low pressure
hot plate set 60 is medium pressure
Hot plate set 120 is high pressure

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B.

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Picture

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low pressure is hot plate off
medium pressure is hot plate set to 60 c
high pressure is hot plate to 120 c

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B.

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B

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zinc does occur

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beaker 2

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B

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I put them in order...
"Low pressure"
"Medium pressure"
"High pressure"

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The answer is false because the larger ice cube is bigger than the smaller ice cubes in the the larger ice cube will not have that much space for the surface.

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B.

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The energy stored in a substance or system is measured in joules (J). When energy is transferred by heating, it can:

change the energy stored in the system

change the physical state of the system

make chemical reactions occur

When energy is transferred to water in the liquid state, water gain kinetic energy and speed up. The larger the mass of water, the more energy needed to raise the temperature by a given amount. This is because more molecules need to have their speed changed.

In the diagram above, the water in the two beakers has been heated by the same Bunsen burner for the same amount of time. This means that the same amount of energy is transferred to both. However, the smaller volume of water increases in temperature more. The same amount of energy has been transferred to a smaller number of particles, so on average each one moves faster than the particles in the other beaker.

Imagine a teaspoon of boiling water at 100°C and a large bowl of water at room temperature (about 20°C):

the teaspoon of water could not melt an ice cube - even though each particle has a greater energy store because there are relatively few of them

the bowl of water could melt an ice cube - even though on average each particle has a smaller energy store because there are many more of them, so the total energy available for transfer is much greater

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Energy and temperature - Energy, temperature and change of state - OCR Gateway - GCSE Physics (Single Science) Revision - OCR Gateway - BBC Bitesize

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The energy stored in a substance or system is measured in joules (J). When energy is transferred by heating, it can: change the energy stored in the system change the physical state of the system make chemical reactions occur When energy is transferred to water in the liquid state, water gain kinetic energy and speed up.

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B.

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hot of plate 120

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Medium pressure:hot plate set to 60 C

high pressure: hot plate set to  120 C

Low pressure:hot plate off

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B

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Beaker 2

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Beaker #2

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B

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zinc sulfide

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When a mixture of zinc and sulfer is heated a chemical Reaction (does occur) . This is supported by the data in the table showing that (Zinc Sulfide is a different color). During this process, the zinc and sulfer atoms (rearrange to form to form new molecules).

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Zinc do occurs

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B.beaker#2

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B

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beaker 2

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B. Beaker #2

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Jashon Answer                                

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Jashon Answer                                

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B

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B.

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B.