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1. Describe the collion theory .
2. Give an example from everday life.
3. What are the factors that affect the rate of a reaction.
4. Discuss th effect of concentration on the rate of a reaction.
5. Make a short quiz of 5 questions.

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1. Describe the collion theory .
2. Give an example from everday life.
3. What are the factors that affect the rate of a reaction.
4. Discuss the effect of surface are on the rate of a reaction.
5. Make a short quiz of 5 questions.

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1. Describe the collion theory .
2. Give an example from everday life.
3. What are the factors that affect the rate of a reaction.
4. Discuss the effect of pressure on the rate of a reaction.
5. Make a short quiz of 5 questions.

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1. Describe the collion theory .
2. Give an example from everday life.
3. What are the factors that affect the rate of a reaction.
4. Discuss the effect of catalyst on the rate of a reaction.
5. Make a short quiz of 5 questions.

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1. Describe the collion theory .
2. Give an example from everday life.
3. What are the factors that affect the rate of a reaction.
4. Discuss the effect of temperature on the rate of a reaction.
5. Make a short quiz of 5 questions.

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Factors That Effect The Rate Of A Reaction

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Factors That Effect The Rate Of A Reaction

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1. Surface area of a solid reactant
In a reaction between a solid and an aqueous/liquid/gas substance, increasing the surface area of the solid-phase reactant increases the number of collisions per second and therefore increases the reaction rate.
By increasing surface area, there are more collisions per unit of time. That's why many solids are powdered using a mortar and pestle before being used in a reaction.

2. Concentration of a reactant
The concentration of a substance can be expressed in a variety of ways depending on the nature of a substance. Aqueous solutions typically have their concentrations expressed in mol/L.
Increasing the concentration of a reactant increases in the number of collisions between the reacting substance per second and therefore increases the reaction rate.
The concentration of an aqueous substance can be increased by simply adding more solute (to make it more concentrated) or adding more solvent (to make it more dilute).

3. Pressure of a reactant
The concentration of a gas is a function of the pressure on the gas. Increasing the pressure of a gas is exactly the same as increasing its concentration. If you have a certain number of gas molecules, you can increase the pressure by forcing them into a smaller volume.
Under higher pressure or at a higher concentration, gas molecules collide more frequently and react at a faster rate. Conversely, increasing the volume of a gas decreases pressure which in turn decreases the collision frequency and thus reduces the reaction rate.
Solids and liquids are not affected by pressure changes.

3. Temperature
With the exception of some precipitation reactions involving ionic compounds in solution, just about all chemical reactions take place at a faster rate at higher temperatures.
A general rule is that a 10°C temperature increase can double a reaction rate. It turns out that the increase in the reaction rate is mainly a function of the more intense collisions. Increased collision frequency is not as significant a factor.

4. Nature of the reactants
Individual properties of substances also affect reaction rates.

5. Presence/absence of a catalyst.

A catalyst is a substance that speeds up a chemical reaction without being chemically changed upon completion of the reaction.
Collisions only result in reactions if the particles collide with enough energy to get the reactions started.
Catalysts help in lowering the activation energy needed for a reaction effectively speeding up the reaction.

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theory used to predict the rates of chemical reactions, particularly for gases. The collision theory is based on the assumption that for a reaction to occur it is necessary for the reacting species (atoms or molecules) to come together or collide with one another. Not all collisions, however, bring about chemical change. A collision will be effective in producing chemical change only if the species brought together possess a certain minimum value of internal energy, equal to the activation energy of the reaction. Furthermore, the colliding species must be oriented in a manner favourable to the necessary rearrangement of atoms and electrons. Thus, according to the collision theory, the rate at which a chemical reaction proceeds is equal to the frequency of effective collisions. Because atomic or molecular frequencies of collisions can be calculated with some degree of accuracy only for gases (by application of the kinetic theory), the application of the collision theory is limited to gas-phase reactions.

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The collision theory is a theory used to measure the rates of reactions, particularly for gases. This theory is based on the assumption that atoms or molecules need to collide with one another in order to create a reaction. However, not all collisions result in a chemical change. In order for a chemical change to occur, the atoms or molecules colliding together need to possess a minimum internal energy, which is equivalent to the activation energy. Because atomic or molecular frequencies of collisions can be calculated with some accuracy for gases, the theory applies only to gases.

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Collision theory provides a qualitative explanation of chemical reactions and the rates at which they occur. A basic principal of collision theory is that, in order to react, molecules must collide.

The molecules in gases and liquids are moving constantly, however only a small number of these collisions lead to the formation of product. For a successful collision, the particles involved must possess the required activation energy, to break some of the existing bonds.

According to collision theory, the rate at which molecules collide will have an impact on the overall reaction rate.

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How does Surface Area affect the Rate of the Reaction?

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How does Surface Area affect the Rate of the Reaction?

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Increasing the surface area of a solid reactant exposes more of its particles. This increases the chances of collisions between reactant particles, so there would be more collisions at any given time, this increasing the rate of the reaction. Note that the mean energy of the particles doesn't change. However, since the frequency of collisions increase, the frequency of successful collisions also increase.

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This is a video on the Collision theory.

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Collision Theory & Reactions Part 1 | Reactions | Chemistry | FuseSchool

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3. What are the factors that affect the rate of a reaction.

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3. What are the factors that affect the rate of a reaction.

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The factors that affect reaction rates are:

surface area of a solid reactant

concentration or pressure of a reactant

temperature

nature of the reactants

presence/absence of a catalyst.

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- concentration of reactants
- Temperature
- Physical state of the reactants
- Dispersion of the reactants
- The solvent
- Presence of a catal

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-  When you cook a big piece of potato, you will take more time compare to the small piece of potato.
- A sugar cube will take more time to melt complete than the sugar powder.

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1. Give one factor that affects the rate of reaction
2. What is collision theory good for?
3. Give an example of the collision theory in everyday life
4. How does surface area affect the rate of reaction?
5. Give an example of a catalyst

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Catalysts increase the rate of reaction without being used up. They do this by lowering the activation energy needed. With a catalyst, more collisions result in a reaction, so the rate of reaction increases. Different reactions need different catalysts.

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The collision theory is used to predict the rates of chemical reaction.Thecollision theory is based on the assumption that for a reaction to occur is isneeded  for a atom or molecule to come together or collide with one another

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Our body system consists lots of biological reactions. If a biochemical reaction in our body is too fast or too slow, it can endanger our life. This is why we use medications.

Another example is photosynthesis,
6 CO₂ + 6 H₂O + light → C​₆H₁₂O₆ + 6 O2.
Plants apply a chemical reaction called photosynthesis to convert carbon dioxide and water into food (glucose) and oxygen.

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https://www.youtube.com/watch?v=-vmQtLpcl48

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1. What is the collision theory?
2. What state of matter does the collision theory relate to the most?
3. What is activation energy?
4. How can you increase the rate of a reaction?
5. Why do more collisions occur when the reaction is heated?

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Surface area
Concentration
Temperature
Presence or absence of a catalyst

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Graph showing how Surface Area affects the rate of a reaction

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Graph showing how Surface Area affects the rate of a reaction

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The collision theory is an assumption that states that for a reaction to occur the elements must come collide together.

If the two molecules

A and B are to react, they must approach closely enough to disrupt some of their existing bonds and to permit the creation of any new ones

Finally, not all collisions are always successful. There needs to be sufficient energy (the right activation energy) and the right orientation.

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1. What are the factors that affect the rate of reactions?

2. In summary, what is the collision theory and what state of matter does it usually apply to?

3. What are everyday examples of the collision theory and can you think of any that were not mentioned?

4. Using the collision theory, how can the rate of reaction be decreased overtime?

5. How will a graph look like if an exothermic reaction took place?

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What are the factors that affect the rate of a reaction?
What is the effect of concentration on the rate of a reaction?

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Then consider everyday examples like cooking. The rate of heat applied while cooking can determine the amount of nutrition that goes into the body.

Also there are examples like genetic reactions, where the rate of reaction determines how an individual can look like and what all characteristics he/she has.

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- Dissolving sugar in tea

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How does temperature effect the rate of reaction?

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How does temperature effect the rate of reaction?

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A higher temperature will increase the rate of reaction as applying heat to a substance will increase the energy of the particles causing them to move around faster colliding with other particles with more force.

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How Surface Area affects the rate of Reaction

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The overall unit links to the global context Orientation in Space and Time as the collision theory developed over time and it was built on previous discoveries. This can also be applied to the orientation of particles in a substance, such as solids that are split apart to increase surface area and the rate of the reaction, or gases in which the collision theory is centered around. There's also a link to orientation in terms of particles, as the factor that dictates whether a chemical or physical change occurs is activation energy, which affects the relationship between the atoms or molecules. Also, the rate of reaction changes over time, with the speed steadily decreasing over time.

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www.quizyourfriends.com/take-quiz.php?id=1901140237043497&lnk&

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Surface area affects the chemical equilibrium by increasing the number of collisions between particles in time and space as the surface area increases. This is because more particles are made available to collisions.

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So basically, when a human collides with a monkey, it forms a banana

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i like donkeys because they remind me of donkey from shrek

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i like donkeys because they remind me of donkey from shrek

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Factors that affect the rate of a reaction

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Factors that affect the rate of a reaction

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SURFACE AREA:
By increasing surface area, there are more collisions per unit of time. That's why many solids are powdered using a mortar and pestle before being used in a reaction.

Examples of other reactions where surface area is important are:

active metals with acids, e.g. HCl with zinc

coal dust with oxygen gas

grain dust with oxygen gas

CONCENTRATION:
Consider the reaction between hydrochloric acid and zinc metal. In terms of the collision theory, collisions between zinc atoms and hydrochloric acid are more frequent with a higher concentration of acid- there is more acid per unit of volume.

PRESSURE:
Increasing the pressure of a gas is exactly the same as increasing its concentration. If you have a certain number of gas molecules, you can increase the pressure by forcing them into a smaller volume. Under higher pressure or at a higher concentration, gas molecules collide more frequently and react at a faster rate. Conversely, increasing the volume of a gas decreases pressure which in turn decreases the collision frequency and thus reduces the reaction rate.

TEMPERATURE
Temperature (in Kelvin degrees) is proportional to the kinetic energy of the particles in a substance. For example, if the Kelvin temperature of a substance is doubled, then the average kinetic energy of the particles in that substance is doubled.
Increasing the temperature causes some of the medium speed molecules to move faster. The result is more molecules with sufficient kinetic energy to collide, increasing the probability of successful collisions.

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For many reactions involving liquids or gases, increasing the concentration of the reactants increases the rate of reaction. In a few cases, increasing the concentration of one of the reactants may have little noticeable effect of the rate.

In the lab, zinc granules react fairly slowly with dilute hydrochloric acid, but much faster if the acid is concentrated.

Solid manganese(IV) oxide is often used as a catalyst in this reaction. Oxygen is given off much faster if the hydrogen peroxide is concentrated than if it is dilute.

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The period of time over which a reaction takes place can be manipulated by changing certain factors of the space in which the reaction is taking place. For example, changing concentration is manipulating the environment and space that the reaction is taking place in. Therefore the time for the reaction will vary according to the change in concentration and will accordingly take more or less time.