Equilibria (triple) quiz

1. State and explain how increasing temperature affects the diffusion of a gas

Gas diffuses slower because the particles collide more often with the air

Gas diffuses slower because the particles have less energy

Gas diffuses quicker because particles have more energy.

Gas diffuses quicker because there is less in its way

Question 1 of 15

2. What is meant by the term endothermic?

A reaction in which heat energy is given out (surroundings get hotter)

A reaction which will only be spontaneous at cold temperatures (below 0⁰C)

A reaction in which heat energy is taken in (surroundings get colder)

A reaction which will only be spontaneous at warm temperatures (above 100⁰C)

Question 2 of 15

3. 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) 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

Question 3 of 15

4. Write a chemical equation for the reaction between hydrogen chloride and ammonia

2NH₃ + 2HCl ⇌ 2NH₃Cl + H₂

NH₃ + HCl ⇌ NH₄Cl + H₂O

2NH₄ + 2HCl ⇌ 2NH₄Cl + H₂

NH₃ + HCl ⇌ NH₄Cl

Question 4 of 15

5. In a sealed container, a reversible reaction can reach a state of ______________________________

Variable equilibrium

Dynamic equilibrium

Constant equilibrium

Static equilibrium

Question 5 of 15

6. What colour is hydrated copper (II) sulfate?

Cream

Purple

White

Blue

Question 6 of 15

7. In the thermal decomposition of calcium carbonate, we might expect 50g of calcium carbonate to produce 28g of calcium oxide. If instead only 24g of calcium oxide is produced, what is the percentage yield?

85.7 %

0.56 %

56 %

0.857 %

Question 7 of 15

8. State two features of a reaction that is in dynamic equilibrium

1) The concentrations of products and reactants are equal. 2) the rate of the forward reaction is equal to the rate of the backward reaction

1) The rate of the forward reaction is equal to the rate of the backward reaction. 2) There is no overall change in concentrations.

1) The equilibrium is on the right hand side producing a greater concentration of product than reactant. 2) The rate of the forward reaction is equal to the rate of the backward reaction

1) The rate of the forward reaction is greater than the rate of the backward reaction. 2) there is no overall change in concentrations

Question 8 of 15

9. Why a catalyst does not affect the position of equilibrium in a reversible reaction?

A catalyst reduces the activation energy, and is not used up

A catalyst has no effect on a forward or backward reactions if it is in dynamic equilibrium

A reaction in dynamic equilibrium already has the lowest possible activation energy

If a reversible reaction is in dynamic equilibrium, a catalyst increases the rate of the forward reaction and the rate of the backward reaction by the same amount, so the position of equilibrium is unaffected

Question 9 of 15

10. What will happen to the equilibrium position when the temperature is decreased? Give a reason for your prediction. CO(g) + 2H₂(g) ⇋ CH₃OH(g) ΔH = –91 kJ mol⁻1

Equilibrium will move to the right because the forward reaction is endothermic

Equilibrium will move to the right because the forward reaction is exothermic

Equilibrium will move to the left because the forward reaction is exothermic

Equilibrium will move to the left because the forward reaction is endothermic

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 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 11 of 15

12. What does the symbol ⇌ mean?

A reaction that requires a catalyst

Variable oxidation state

Reversible reaction

Equal amounts of reactants and products

Question 12 of 15

13. What does the symbol ΔH mean

exothermic

heat energy

specific heat capacity

enthalpy (energy) change

Question 13 of 15

14. What is meant by the term activation energy?

The minimum energy that the particles in collision must have if a reaction is going to occur

The maximum energy of the final product for it to be stable

The energy released by the reaction

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

Question 14 of 15

15. In a calorimetry experiment to investigate the heat energy released by the combustion of ethanol, why should the water in the calorimeter be stirred?

To ensure the container does not get too hot

To allow the heat to spread evenly through the copper container

To ensure the heat energy is mixed evenly throughout all the water

To prevent the water from evaporating

Question 15 of 15

Equilibria (triple) quiz

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