Rate of Reaction Quiz GCSE – Educational Consultant, High Performance Coach to Executives & Entrepreneurs, Family Life Expert, Teachers. Coach & Staff Devpmt Trainer

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#1. What does “rate of reaction” mean?

a) How many bubbles are made

b) How fast reactants become products

c) How hot the reaction is

d) How much product is made

#2. Which of these does NOT increase the rate of reaction?

a) Lower temperature

b) Crushing solids

c) Using a catalyst

d) Increasing pressure

#3. What happens to particles when you heat them up?

a) They slow down

b) They break apart

c) They move faster and collide more

d) They disappear

#4. Which of the following would slow down a reaction?

a) Increasing the temperature

b) Decreasing the concentration

c) Crushing a solid

d) Adding a catalyst

#5. Which factor affects only gas reactions, not solids or liquids?

a) Temperature

b) Pressure

c) Catalyst

d) Concentration

#6. What is a catalyst?

a) A chemical that reacts and disappears

b) A substance that speeds up a reaction without being used up

c) A type of acid

d) A gas made during a reaction

#7. A student reacts marble chips with hydrochloric acid. Which change would make the reaction happen faster?

a) Use smaller marble chips

b) Use colder acid

c) Use less acid

d) Remove the catalyst

#8. Which of these shows a fast reaction on a rate graph?

a) A flat horizontal line

b) A steep curve that flattens quickly

c) A line that never changes

d) A slow rising line

#9. In the reaction between magnesium and hydrochloric acid, gas is produced. How could you measure the rate?

a) Check the colour of the acid

b) Measure the temperature drop

c) Measure the volume of gas produced over time

d) Weigh the magnesium before and after

#10. Why does increasing surface area increase the rate of reaction?

a) It makes particles heavier

b) More particles are exposed to collide

c) It changes the temperature

d) It removes impurities

#11. Which of the following statements is TRUE?

a) Only liquids can have fast reactions

b) Gases do not react with solids

c) Reactions happen faster if there are more collisions between particles

d) Increasing pressure slows reactions down

#12. A student adds a catalyst to a reaction. What effect will it have?

a) It will change the colour

b) It will speed up the reaction

c) It will increase temperature

d) It will form more products

#13. “A catalyst gets used up during a reaction.”

True

False

#14. Why does powdered marble react faster than large lumps?

#15. Why does increasing concentration increase the rate?

#16. Two students react magnesium with hydrochloric acid. Student A uses 1M acid, Student B uses 2M acid. Who gets a faster reaction? Why?

Student A

Student B

None

#17. In an experiment, the graph for a reaction starts steep and then flattens out. What does that show?

#19. What name is given to the minimum amount of energy needed by particles for them to react when they collide?

Activation energy

Catalytic energy

Threshold energy

#20. What is the name of the model which is used to explain how different factors affect the rate of a reaction?

Particle Theory

Collision theory

Big Bang Theory

#21. What piece of apparatus could be used to measure the volume of gas produced in a reaction

Beaker

Test tube

Gas syringe

#22. Which of the following is a possible unit for rate of reaction?

cm3/s

m/s

#23. Which of the following would speed up a reaction?

Using lumps instead of powder

Increasing the concentration of an acid

Decreasing the temperature

#24. Which of the following will increase the frequency of successful collisions?

Decreasing the pressure

Decreasing the concentration

Increasing the temperature

#25. Which of the following has the smallest surface area to volume ratio?

Powder

Gauze

Lumps

#26. Which of the following statements about catalysts is false?

They speed up reactions

They become chemically changed at the end of the reaction

They provide an alternative reaction pathway with a lower activation energy

#27. Which of the following will increase the proportion of successful collisions?