Kinetics quiz

1. 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 1 of 15

2. 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 less steeply. Levels out at same level.

Lines falls more steeply. Levels out at same level.

Question 2 of 15

3. 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 3 of 15

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

Rate of reaction decreases

Rate of reaction is unaffected

Reaction stops

Rate of reaction increases

Question 4 of 15

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

4H₂O₂ → 2H₂O + O₂

2H₂O₂ → 2H₂O + O₂

H₂O₂ → 2H₂O + O₂

H₂O₂ → H₂O + O₂

Question 5 of 15

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

No reaction

The particles fuse together

The reaction only goes partway

The reaction still occurs but very slowly

Question 6 of 15

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

Potassium permanganate (VII), KMnO₄

Manganese (IV) oxide, MnO₂

Magnesium (II) oxide, MgO₂

Vanadium (V) oxide V₂O₅

Question 7 of 15

8. 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) decrease 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) increase rate of reaction

Question 8 of 15

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

Catalyst

Reagent

Ore

Solute

Question 9 of 15

10. What is a catalyst?

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 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

Question 10 of 15

11. Explain how a catalyst works

A catalyst provides an alternative pathway with lower activation energy

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

Question 11 of 15

12. 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.

No change. Line would look the same.

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

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

Question 12 of 15

13. 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

Ethene of various concentrations reacted with water to make ethanol

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

Question 13 of 15

14. 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) more 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) less frequent collisions 3) decrease rate of reaction

Question 14 of 15

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

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

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

Question 15 of 15

Kinetics quiz

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