Kinetics quiz

1. 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 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 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

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

Question 2 of 15

3. 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 speeds up 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 3 of 15

4. Explain how a catalyst works

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

A catalyst reduces the activation energy of the reaction

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

Question 4 of 15

5. 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) decrease rate of reaction

1) more particles in same space 2) less frequent collisions 3) increase 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 5 of 15

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

The particles fuse together

The reaction only goes partway

No reaction

The reaction still occurs but very slowly

Question 6 of 15

7. 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 twice the height of the original.

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.

No change. Line would look the same.

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

Question 7 of 15

8. 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 a level twice as high as the original.

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.

Question 8 of 15

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

hydrogen peroxide → water + oxygen + carbon dioxide

hydrogen peroxide → hydrogen + oxygen + carbon dioxide

hydrogen peroxide → water + oxygen

hydrogen peroxide → water + hydrogen

Question 9 of 15

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

Increase surface area (solids), increase 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), decrease 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 10 of 15

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

water

hydrogen peroxide

manganese oxide

magnesium oxide

Question 11 of 15

12. 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 12 of 15

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

Catalyst

Ore

Reagent

Solute

Question 13 of 15

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

Rate of reaction is unaffected

Reaction stops

Rate of reaction increases

Rate of reaction decreases

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

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

Large chips or powdered sodium nitrate added to hydrochloric acid

Question 15 of 15

Kinetics quiz

Kinetics quiz

Related Posts:

Share This Story, Choose Your Platform!