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

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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) 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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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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1) What is a catalyst?
2) How does a catalyst work?
3) How does a catalyst increase the rate of reaction?

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Catalyst

1) What is a catalyst?

A catalyst is a substance that speeds up a chemical reaction without being used up or permanently changed at the end of the reaction.

2) How does a catalyst work?

A catalyst works by providing an alternative reaction pathway that requires less energy than the uncatalysed reaction.

The catalyst may temporarily react with the reactants.

It forms intermediate steps that are easier to complete.

After the reaction, the catalyst is regenerated and can be used again.

3) How does a catalyst increase the rate of reaction?

A catalyst increases the rate of reaction by lowering the activation energy (the minimum energy needed for a reaction to start).

Because of this:

More particles have enough energy to react.

More successful collisions occur per second.

The reaction happens faster.

A catalyst does not change:

The overall energy change of the reaction

The final products
It only changes how fast the reaction happens.

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1) If the particle size is smaller, the surface area to volume ratio increases.

2) When there is a higher surface area to volume ratio, more particles will be in contact with the acid and react. Thus the rate of reaction is higher.

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An increase of pressure in gases gives less space for the gas molecules to move in random directions. This increases the rate of reaction as molecules will collide with each other more efficiently.

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1) When the pressure is increased, there will be a higher average number of collisions between particles in the space as there is less room for gas particles to move.

2) When the pressure increases in a system with gaseous reactants, they will start to collide with each other more often, allowing quicker reaction times.

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1) As the increase of pressure would force the gas particles to be closer to each other and since gases have a lower activation energy cost compared to solids and liquids, the rate of reaction would be higher.

2) The rate of reaction would be higher as there would be more effective collisions between gas molecules inside the system

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A significant increase in pressure would allow for less space for gas molecules to move around freely. This thus increases the rate of reaction as there will be more effective collision of molecules.

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1) The particles will gain energy and move faster.

2) The collisions will be effective.

3) The rate of reaction will be higher.

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2) 2moldm-3 acid. it has more h+ ions per dm-3 so there are more frequent collisions between acid and metal ions, so there is higher rate of reaction

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Joshua Soh, Jaden Oh, Nat Kwan, Ethan Szie

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Joshua Soh, Jaden Oh, Nat Kwan, Ethan Szie

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Q1: As particle size decreases, the exposed surface area for all particles of that type increases.

Q2: As particle size decreases, the surface area of particles exposed for collisions to occur increases. This increases the frequency of effective collisions between the reactant particles, leading to a higher rate of reaction.

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1)The 2mol per dm cube acid is twice as concentrated as the 1 mol per dm cube acid.

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1) Difference between 1 mol dm⁻³ and 2 mol dm⁻³ acid

1 mol dm⁻³ means 1 mole of acid particles in 1 dm³ (1 litre) of solution.

2 mol dm⁻³ means 2 moles of acid particles in 1 dm³ (1 litre) of solution.

So, 2 mol dm⁻³ is twice as concentrated as 1 mol dm⁻³.
It contains double the number of acid particles (and hydrogen ions, H⁺) in the same volume.

2) Same volume of each acid reacts with the same mass of metal

Which reacts faster?

Reaction speed depends on how often acid particles collide with the metal.

The 2 mol dm⁻³ acid has more particles per unit volume, so:

More frequent collisions

More successful collisions

✅ 😁Therefore, the 2 mol dm⁻³ acid reacts faster than the 1 mol dm⁻³ acid.

Summary

Difference: 2 mol dm⁻³ is more concentrated than 1 mol dm⁻³.

Faster reaction: 2 mol dm⁻³ acid, because it has more acid particles.