Kinetics quiz

1. Explain how a catalyst works

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

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

Question 1 of 15

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

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

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

Marble chips added to hydrochloric acid of various concentrations

Ethene of various concentrations reacted with water to make ethanol

Question 2 of 15

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

Ore

Reagent

Catalyst

Solute

Question 3 of 15

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

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

Question 4 of 15

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

Manganese (IV) oxide, MnO₂

Potassium permanganate (VII), KMnO₄

Magnesium (II) oxide, MgO₂

Vanadium (V) oxide V₂O₅

Question 5 of 15

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

Rate of reaction decreases

Reaction stops

Rate of reaction increases

Rate of reaction is unaffected

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

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

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

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

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

Question 8 of 15

9. What happens to the rate of reaction if the temperature is INCREASED?

Rate of reaction increases

Rate of reaction is unaffected

Rate of reaction decreases

Reaction stops

Question 9 of 15

10. 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

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

Large chips or powdered sodium nitrate added to hydrochloric acid

Question 10 of 15

11. What is a catalyst?

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

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

Question 11 of 15

12. 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 less steeply. Levels out at lower level.

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

Line rises more steeply. Levels out at higher level.

Line rises more steeply. Levels out at same level.

Question 12 of 15

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

manganese oxide

magnesium oxide

water

hydrogen peroxide

Question 13 of 15

14. 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 14 of 15

15. 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.

Line rises more steeply. Levels out at same level.

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

No change. Line would look the same.

Question 15 of 15

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