Kinetics quiz

1. On a graph showing gas produced (vertical axis) over time (horizontal axis), how does the line tell us the rate of reaction?

The longer the line, the slower the rate of reaction

The steeper the line, the slower the rate of reaction

The steeper the line, the faster the rate of reaction

The longer the line, the faster the rate of reaction

Question 1 of 15

2. Explain the effects of increasing the temperature on the rate of a reaction in terms of particle collision theory

1) particles have less kinetic energy 2) less frequent collisions 3) and a lower proportion of the collisions which occur have greater or equal to the activitation energy 4) decrease rate of reaction

1) particles have more kinetic energy 2) more frequent collisions 3) and a higher proportion of the collisions which occur have greater or equal to the activation energy 4) increase rate of reaction

1) particles have more kinetic energy 2) more frequent collisions 3) and a lower proportion of the collisions which occur have greater or equal to the activitation energy 4) increase rate of reaction

1) particles have less kinetic energy 2) less frequent collisions 3) and a lower proportion of the collisions which occur have greater or equal to the activitation energy 4) increase rate of reaction

Question 2 of 15

3. Explain the effects of increasing the surface area of a solid on the rate of a reaction in terms of particle collision theory

1) more particles exposed 2) more frequent collisions 3) increase rate of reaction

1) more particles exposed 2) less frequent collisions 3) decrease rate of reaction

1) more particles exposed 2) more frequent collisions 3) decrease rate of reaction

1) more particles exposed 2) less frequent collisions 3) increase rate of reaction

Question 3 of 15

4. Give a simple reaction can be used to investigate the effect of changing concentration on the rate of reaction

Iron ore of various concentrations reacted via the displacement method to produce iron

Ethene of various concentrations reacted with water to make ethanol

Sodium hydroxide of various concentrations added to hydrochloride acid to produce sodium chloride

Marble chips added to hydrochloric acid of various concentrations

Question 4 of 15

5. Explain how a catalyst works

A catalyst increases the surface area of the reagents to increase the rate of reaction

A catalyst increases the concentration of the reagents by taking up water to increase the rate of reaction

A catalyst reduces the activation energy of the reaction

A catalyst provides an alternative pathway with lower activation energy

Question 5 of 15

6. Calcium carbonate reacts with an excess of hydrochloric acid in a flask. The volume of carbon dioxide given off is measured in a gas syringe. This is shown on the graph. How would the graph look different if the reaction was done with twice the volume of the acid?

Line rises more steeply. Levels out at same level.

Line rises at the same rate, but levels out at twice the height.

No change. Line would look the same.

Line rises more steeply. Levels out at a level twice as high as the original.

Question 6 of 15

7. What reactant is used to produce a sample of oxygen in the lab?

manganese oxide

water

magnesium oxide

hydrogen peroxide

Question 7 of 15

8. What is a catalyst?

A substance that helps dissolve insoluble reagents to speed up the rate of reaction

A substance that slows down a chemical reaction but is chemically unchanged at the end of the reaction

A substance that speeds up a chemical reaction but is used up as the reaction proceeds

A substance that speeds up a chemical reaction but is chemically unchanged at the end of the reaction

Question 8 of 15

9. What happens if two particles collide with less than the activation energy

The particles fuse together

No reaction

The reaction only goes partway

The reaction still occurs but very slowly

Question 9 of 15

10. What is meant by the term activation energy?

The energy released by the reaction

The energy provided by the catalyst to allow a reaction to proceed

The maximum energy of the final product for it to be stable

The minimum energy that the particles in collision must have if a reaction is going to occur

Question 10 of 15

11. Calcium carbonate reacts with an excess of hydrochloric acid in a flask. The mass of flask and contents decreases over time as the carbon dioxide escapes. This is shown on the graph. How would the graph look different if the reaction was done with a lower concentration of hydrochloric acid?

Lines falls more steeply. Levels out at higher level.

Lines falls less steeply. Levels out at same level.

Lines falls more steeply. Levels out at same level.

Lines falls more steeply. Levels out at lower level (but still above zero).

Question 11 of 15

12. What type of substance speeds up a chemical reaction but is chemically unchanged at the end of the reaction?

Solute

Catalyst

Reagent

Ore

Question 12 of 15

13. Give a simple reaction can be used to investigate the effect of changing surface area on the rate of reaction

Burning powdered magnesium or strips of magnesium in air

Large chips or powdered sodium nitrate added to hydrochloric acid

Hydrochloric acid added to either marble chips or powdered calcium carbonate

Large chips or powdered ion ore reacted to produce iron using the displacement method

Question 13 of 15

14. Write the chemical equation for the decompostion of hydrogen peroxide, H₂O₂

4H₂O₂ → 2H₂O + O₂

2H₂O₂ → 2H₂O + O₂

H₂O₂ → 2H₂O + O₂

H₂O₂ → H₂O + O₂

Question 14 of 15

15. What happens to the rate of reaction if the pressure of gases is INCREASED?

Reaction stops

Rate of reaction increases

Rate of reaction is unaffected

Rate of reaction decreases

Question 15 of 15

Kinetics quiz

Related Posts:

Share This Story, Choose Your Platform!