Kinetics quiz

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

Reaction stops

Rate of reaction decreases

Rate of reaction increases

Rate of reaction is unaffected

Question 1 of 15

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

The steeper the line, the faster the rate of reaction

The longer the line, the slower the rate of reaction

The longer the line, the faster the rate of reaction

The steeper the line, the slower the rate of reaction

Question 2 of 15

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

Ethene of various concentrations reacted with water to make ethanol

Marble chips added to hydrochloric acid of various concentrations

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

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

Question 3 of 15

4. What is a catalyst?

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 chemically unchanged at the end of the reaction

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

Question 4 of 15

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

Solute

Catalyst

Reagent

Ore

Question 5 of 15

6. Write the word equation for the decompostion of hydrogen peroxide, H₂O₂

hydrogen peroxide → water + oxygen

hydrogen peroxide → water + hydrogen

hydrogen peroxide → water + oxygen + carbon dioxide

hydrogen peroxide → hydrogen + oxygen + carbon dioxide

Question 6 of 15

7. What is meant by the term activation energy?

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

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

The energy released by the reaction

Question 7 of 15

8. Describe the laboratory preparation of oxygen from hydrogen peroxide

Hydrogen peroxide is added to a flask containing a catalyst of magnesium oxide, MgO₂. Oxygen is produced and is collected underwater.

Hydrogen peroxide is added to a flask containing a catalyst of nickel oxide, NiO₃. Oxygen is produced and is collected underwater.

Hydrogen peroxide is added to a flask containing a catalyst of manganese oxide, MnO₂. Oxygen is produced and is collected underwater.

Hydrogen peroxide is added to a flask containing a catalyst of vanadium oxide, V₂O₅. Oxygen is produced and is collected underwater.

Question 8 of 15

9. 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 9 of 15

10. Hydrochloric acid reacts with an excess of calcum carbonate 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 the same volume of acid, but with an acid which is twice as concentrated?

The line would rise more steeply, and finish at a higher level than the original, but how much higher would depend on whether the calcium carbonate were still in excess.

The line would rise at the same rate, but finish at twice the height of the original.

No change. Line would look the same.

The line would rise more steeply, and finish at a twice the height of the original.

Question 10 of 15

11. 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) decrease 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 11 of 15

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

No reaction

The reaction still occurs but very slowly

The particles fuse together

The reaction only goes partway

Question 12 of 15

13. 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) less frequent collisions 3) increase rate of reaction

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

Question 13 of 15

14. Large chips of 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 a powdered calcium carbonate?

Line rises more steeply. Levels out at higher level.

Line rises more steeply. Levels out at same level.

Line rises less steeply. Levels out at lower level.

Line rises at same rate, but levels out at a higher level.

Question 14 of 15

15. 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

Burning powdered magnesium or strips of magnesium in air

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

Question 15 of 15

Kinetics quiz

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