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1) Why would an increase of pressure cause a significant change in the rate of reaction of gases, compared to solids and liquids?
2) What happens when you increase pressure in a system containing gaseous reactants?

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A) View this video How to speed up chemical reactions (and get a date) - Aaron Sams - YouTube
B) Write your group number and names of group members.
C) Discuss the questions and answer as a group. 1 person to key in the answers.
D) Nominate a spokesman to present the answers.
D) You are given 7 mins for this activity.

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How to speed up chemical reactions (and get a date) - Aaron Sams

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1) What happens to the particles when you increase the temperature of the system?
2) What type of collision will result when reacting particles achieve its activation energy?
3) What is the effect on the rate of reaction when you increase the temperature of the system?

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You were given an acid of 2 different concentrations -
1 moldm-3 and 2 moldm⁻³
1) What is the difference between 1 moldm-3 and 2 moldm⁻³ of acid?
2) The same volume of the acids  was reacted with the same mass of metal. Which would react faster? Why?

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1) How is particle size related to its surface area?
2) Explain how particle size affect rate of reaction.

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1) 1 moldm-3

2) 2 moldm-3 because it has a higher concentration, thus more will react at any given time.

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1 . 1 mol dm^(-3)

2. the 2 mol dm^(-3) acid solution would likely react faster with the same mass of metal compared to the 1 moldm^(-3) acid solution due to its higher concentration.

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the particles in the system gain kinetic energy and start to move about more

effective collision

When u increase the temperature, the particles will gain kinetic energy. This will increase the rate of effective collisions and hence increase the rate of reaction.

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1) Increasing pressure would could make the volume decrease, hence making the molecules forced to collide and react with one another

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Q1. The more the particles break apart, the larger the surface area.

Q2. The smaller the particle size the faster the reaction.

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1. Since gas is compressible, their volume can be reduced by a large amount under pressure. As such, whenthe pressure increases, there will be a higher concentration of gas particle within an unit volume.

2. Increasing pressure will lead to an increased reaction rate, and may result in changes of volume, which results in change of rate of reactants.

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Q1. As the particle size decreases, the surface area per unit mass or volume increases

Q2. Smaller particle size increases surface area, accelerates collisions, and enhances reaction rates due to increased contact and diffusion.

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Q1. The smaller the particle, the smaller the surface area.

Q2. A smaller particle size means smaller surface area, which decreases rate of reaction.