Kinetics quiz

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

Reagent

Solute

Catalyst

Ore

Question 1 of 15

2. 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 2 of 15

3. 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 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 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

Question 3 of 15

4. 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 less steeply. Levels out at same level.

Lines falls more steeply. Levels out at same level.

Lines falls more steeply. Levels out at lower level (but still above zero).

Lines falls more steeply. Levels out at higher level.

Question 4 of 15

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

Manganese (IV) oxide, MnO₂

Vanadium (V) oxide V₂O₅

Potassium permanganate (VII), KMnO₄

Magnesium (II) oxide, MgO₂

Question 5 of 15

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

hydrogen peroxide → hydrogen + oxygen + carbon dioxide

hydrogen peroxide → water + hydrogen

hydrogen peroxide → water + oxygen

hydrogen peroxide → water + oxygen + carbon dioxide

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 more steeply. Levels out at same level.

No change. Line would look the same.

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

Line rises at the same rate, but levels out at twice the height.

Question 7 of 15

8. 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 reduces the activation energy of the 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 8 of 15

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

Rate of reaction decreases

Rate of reaction is unaffected

Rate of reaction increases

Reaction stops

Question 9 of 15

10. What simple change could be made to a reaction to speed it up dramatically?

Decrease the pressure

Heat it up

Decrease the concentration

Decrease the surface area

Question 10 of 15

11. 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 used up as the reaction proceeds

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

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. 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 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 or equal to the activation energy

Question 13 of 15

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

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

Large chips or powdered sodium nitrate added to hydrochloric acid

Burning powdered magnesium or strips of magnesium in air

Hydrochloric acid added to either marble chips or powdered calcium carbonate

Question 14 of 15

15. Explain the effects of increasing the concentration of solutions 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) less frequent collisions 3) decrease rate of reaction

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

Question 15 of 15

Kinetics quiz

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