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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. Relate your factor to the global context
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 th effect of TEMPERATURE AND 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 th effect of PRESSURE AND SURFACE AREA on the rate of a reaction.
5. Make a short quiz of 5 questions.

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The affect of pressure and surface area on the rate of a reaction:
Surface Area:
Increasing the surface area of the reactants exposes more of its particles to attack. This results in an increased chance of collisions between reactant particles, so there are more collisions in any given time and the rate of reaction increase.
If the surface area to volume ratio of a reacting solid is increased: more reactant particles are exposed at the surface. the frequency of collisions between reactant particles increases
Pressure:
Increasing the pressure on a reaction involving reacting gases increases the rate of reaction. Changing the pressure on a reaction that involves only solids or liquids has no effect on the rate. If there are more molecules in a smaller volume, the chances of collision are greater, and the rate increases.

Quiz:
1) How does pressure affect the rate of the reaction?
2) How does surface area affect the rate of the reaction?
3) Can you think of a reaction that would be affected by surface are and pressure?
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When the temperature in a system (i.e. the place where a reaction takes place) increases, the rate of a reaction increases. Temperature is the average kinetic energy contained in the particles, thus when the temperature increases, we deduce that the average kinetic energy increases as well. When there's more kinetic energy, the particles move faster as well, so there's a greater chance for successful collisions between the appropriate reactants and atoms. For example, cooking a dish will take shorter time when placed upon a strong flame, rather than a weaker flame. The collisions between the ingredients will increase, creating the product faster.

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In a chemical reaction, the reactant particles can only react with each other when they bump into one another. According to collision theory when molecules collide bonds between their atoms can break, and then new bonds can form to make new molecules.

The molecules in gases and liquids are moving constantly, and millions of collisions take place every second. But only a small number of these collisions lead to the formation of product. For a collision to be 'successful', the particles involved must possess enough energy, called the activation energy, to break some of the existing bonds.

Any change that increases the number of collisions per second, or increases the energy of the particles that are colliding, will increase the rate of reaction.

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For any collision to occur, there have to be some energy applied to the particles for them to have successful collisions and break the bonds of other atoms, to create products. The minimal required energy is called the activation energy, and the catalyst provides an alternative way to a reaction. The particles which don't have enough of the activation energy can now have a different way to react.

Think about it as a mountain between two valleys, and the only way to get from one valley to another is over the mountain. Only the most active and the ones with the most energy are the ones capable of climbing over the mountain. Now, suppose a tunnel is built beneath the mountain, providing a direct way to the other valley. More people will be able to take this easier route. A catalyst essentially does this. It doesn't lower the level of the mountain (or the activation energy), it just provides a different way.

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When cars moving at a high speed collide with one another, the result can be a particularly dramatic change. A high energy collision can convert a functional car into a pile of scrap metal and spare parts. On the other hand, a slower, low energy collision might just cause a scratch or a minor dent.

With relation to an example for the use of concentration to increase the rate of a reaction; when the acidity levels of our stomachs increase, antacid tables are taken in order the reduce the acidity level in order for us to function normally. Therefore, when 2 tablets of antacid are used, the tablet will neutralize the same amount of acid faster that just one tablet, because we increase the amount of reactant (concentration). Additionally, we could also take a pill that consists of a higher concentration of each substance in the tablet and as a result the neutralization reaction with take place faster.

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Effect of Concentration on the Rate of a Reaction

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Effect of Concentration on the Rate of a Reaction

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Increasing the concentration means that we have more particles in the same volume of solution which increases the rate of reaction because more of the reacting molecules or ions are present to form the reaction products. This is especially true when concentrations are low and few molecules or ions are reacting.This increases the chance of collisions between reactant particles, resulting in more collisions in any given time and a faster reaction.

For example, in the reaction between magnesium and hydrochloric acid, the magnesium is introduced as a solid while the hydrochloric acid is in solution. Typically the acid reacts with magnesium atoms from the metal, and as the metal is eaten away, the reaction proceeds. When more hydrochloric acid is in solution and the concentration is higher, more hydrochloric acid ions eat away at the metal and the reaction speeds up.

In relation to the global context (Orientation in space and time), concentration is one of the factors that determines how quickly a reaction occurs and the time it takes to form a product. With reference to space, when the concentration of a substance is increased, more atoms and ions are present, thereby reducing the space and increasing the chances of collisions to increase the rate of the reaction as a whole. Lastly, orientation is applied to the collision theory where collisions cannot occur if the atoms are not in the right orientation to be able to collide fast enough and form a reaction.

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1) Which two factors affect the number of collisions that take place in relation to the collision theory?
2) State one example from the real life where the collision theory is applicable
3) How does increasing the concentration of a substance increase the rate of a reaction?
4) In which circumstance, would increasing the concentration not increase the rate of a reaction?
5) State a real-life application where increasing the concentration can benefit a situation?