Kinetics quiz

1. State the catalyst used for making oxygen through the decomposition of hydrogen peroxide

Vanadium (V) oxide V₂O₅

Potassium permanganate (VII), KMnO₄

Manganese (IV) oxide, MnO₂

Magnesium (II) oxide, MgO₂

Question 1 of 15

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

Marble chips added to hydrochloric acid of various concentrations

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

Ethene of various concentrations reacted with water to make ethanol

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

Question 2 of 15

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

water

hydrogen peroxide

magnesium oxide

manganese oxide

Question 3 of 15

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

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

Burning powdered magnesium or strips of magnesium in air

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 reduces the activation energy of the reaction

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

A catalyst provides an alternative pathway with lower activation energy

Question 5 of 15

6. What happens to the rate of reaction if a catalyst is added?

Rate of reaction increases

Rate of reaction decreases

Rate of reaction is unaffected

Reaction stops

Question 6 of 15

7. 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 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.

Line rises more steeply. Levels out at same level.

Question 7 of 15

8. With how much energy must two particles collide for a reaction to occur?

The particles must collide with an energy greater than or equal to the activation energy

The particles must collide with an energy equal to the activation energy

The particles must collide with an energy less than the activation energy

The particles must collide with an energy greater than the activation energy

Question 8 of 15

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

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 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 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

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

Question 9 of 15

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

Reagent

Solute

Ore

Catalyst

Question 10 of 15

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

No reaction

The reaction still occurs but very slowly

The reaction only goes partway

The particles fuse together

Question 11 of 15

12. Explain the effects of increasing the pressure of gases on the rate of a reaction in terms of particle collision theory

1) more particles in same space 2) less frequent collisions 3) increase rate of reaction

1) more particles in same space 2) less frequent collisions 3) decrease rate of reaction

1) more particles in same space 2) more frequent collisions 3) increase rate of reaction

1) more particles in same space 2) more frequent collisions 3) decrease rate of reaction

Question 12 of 15

13. State 5 ways in which the rate of reaction could be increased

Increase surface area (solids), decrease temperature, increase concentration (solutions), increase pressure (gases), add an appropriate catalyst

Increase surface area (solids), increase temperature, increase concentration (solutions), decrease pressure (gases), add an appropriate catalyst

Increase surface area (solids), increase temperature, increase concentration (solutions), increase pressure (gases), add an appropriate catalyst

Increase surface area (solids), decrease temperature, increase concentration (solutions), decrease pressure (gases), add an appropriate catalyst

Question 13 of 15

14. 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 lower level (but still above zero).

Lines falls more steeply. Levels out at higher level.

Lines falls more steeply. Levels out at same level.

Lines falls less steeply. Levels out at same level.

Question 14 of 15

15. What is a catalyst?

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

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

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

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

Question 15 of 15

Kinetics quiz

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