Starter quiz
- In the following reaction identify the reactant: hydrogen peroxide → water + oxygen
- hydrogen peroxide ✓
- hydrogen
- water
- oxygen
- energy
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- Which solution has the highest concentration?
- 0.5 g/cm³
- 1.0 g/cm³
- 2.0 g/cm³ ✓
- 0.1 g/cm³
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- Which of the following statements about rate of reaction are true?
- It is the speed with which a chemical reaction takes place. ✓
- It can be measured by the amount of reactant used × time taken.
- It can be measured by the amount of reactant used ÷ time taken. ✓
- It can be measured by the amount of product formed.
- It can be measured by the amount of product formed × time taken.
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- A student has 5 g of calcium carbonate. How can they increase the surface area of the calcium carbonate?
- heat the calcium carbonate
- use a mass of 10 g of calcium carbonate
- increase the density of the calcium carbonate
- crush the calcium carbonate ✓
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- On a volume versus time graph, what does a steep gradient represent?
- a high rate of reaction ✓
- the rate of reaction is zero
- a low rate of reaction
- the rate of reaction is not affected by the variable
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- Match the key term to the correct definition.
- collision theory⇔particles must collide, and with sufficient energy, in order to react ✓
- activation energy⇔the minimum energy that the particles must have in order to react ✓
- concentration⇔the amount of chemical dissolved in a certain volume of solution ✓
- surface area⇔is the total area of every outer surface of an object ✓
Exit quiz
- Which conditions must particles of reactants meet in order to react in a chemical rection?
- they must be in a liquid state
- they must be in a gaseous state
- they must have similar energy
- they must collide with sufficient energy ✓
- thy must be at a high concentration
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- How does increasing the surface area of a solid affect the rate of reaction?
- it decreases the rate of reaction
- it increases the rate of reaction ✓
- it has no effect on the rate of reaction
- it changes the colour of the reaction
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- Why does increasing the concentration of reactants typically increase the rate of reaction?
- it increases the size of the reactant particles
- it decreases the number of successful collisions
- it increases the number of successful collisions
- it decreases the speed of reactant particles
- it increases the frequency of successful collisions ✓
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- What happens when the concentration of a reacting solution is increased?
- the reactant particles are more likely to collide ✓
- the speed of particles decreases
- the particles are more spread out
- the reaction becomes slower
- there are more reactant particles in the same volume ✓
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- What effect does decreasing the pressure of reacting gases have on the rate of reaction?
- it increases the frequency of collisions
- the particles move closer together
- it increases the pressure of the gases
- it decreases the frequency of collisions ✓
- more particles have energy higher than the activation energy
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- What effect does increasing the temperature of reactants have on the rate of reaction?
- it decreases the speed of particles
- it increases the kinetic energy of particles ✓
- it decreases the number of collisions
- it increases the frequency of successful collisions ✓
- it increases the number of particles exposed on the surface of a solid reactant
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Worksheet
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Presentation
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Video
Lesson Details
Key learning points
- Particles of reactants in a chemical reaction can react together if they collide with sufficient energy.
- Increasing surface area of a solid lets more reacting particles in a solution collide with its particles each second.
- Increasing concentration of a reacting solution introduces more reactant particles, so they collide more frequently.
- Increasing temperature of reactants increases the speed of particles, so they collide more frequently.
- Increasing pressure of reacting gases pushes reactant particles closer together, so they collide more frequently.
Common misconception
That every collision between reactant particles results in a chemical reaction.
The slide deck addresses that not every collision between reactant particles results in a chemical reaction. The particles must collide with the activation energy in order for the collision to be successful and a new product be formed.
Keywords
Collision theory - The collision theory is that particles must collide, and with sufficient energy, in order to react.
Activation energy - The minimum energy that the particles must have in order to react is known as the activation energy.
Rate of reaction - Rate of reaction is the speed with which a chemical reaction takes place, measured by the amount of a reactant used or amount of product formed in a given time.
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