Reversible Reactions Quiz Questions And Answers

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  • 1/7 Questions

    2NH3(g) <------>  N2(g) + 3H2(g) ;  Heat of reaction = +92 kJThe amount of ammonia in the equilibrium mixture can be made larger by

    • Changing the catalyst.
    • Lowering the temperature.
    • Lowering the pressure.
    • Removing some of the hydrogen.
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About This Quiz

A reversible reaction is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back. Are you preparing for exams on the subject? This quiz will help you do that.

Reversible Reactions Quiz Questions And Answers - Quiz

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  • 2. 

    When a reversible reaction reaches dynamic equilibrium at constant temperature,

    • The reaction stops.

    • Equal amounts of reactants and products are present.

    • The ratio of the product concentration to the reactant concentration is constant.

    • The products of the forward reaction stop reacting altogether.

    Correct Answer
    A. The ratio of the product concentration to the reactant concentration is constant.
    Explanation
    When a reversible reaction reaches dynamic equilibrium at a constant temperature, it means that the rate of the forward reaction is equal to the rate of the reverse reaction. This implies that the concentrations of the reactants and products remain constant over time. At equilibrium, the ratio of the product concentration to the reactant concentration is constant, indicating that the reaction has reached a balance where the concentrations of the reactants and products are stable. Therefore, the correct answer is that the ratio of the product concentration to the reactant concentration is constant.

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  • 3. 

    The equation shows the equilibrium between A, B and C.A (g) + 2 B (g)  <--->  2 C (g)       ΔH = +150 kJHow can the amount of B in the equilibrium mixture be increased?

    • Adding more of A

    • Lowering the temperature

    • Removing some of C

    • Increasing the pressure

    Correct Answer
    A. Lowering the temperature
    Explanation
    Lowering the temperature will shift the equilibrium towards the reactants side to counteract the decrease in temperature. Since the forward reaction is exothermic (ΔH = +150 kJ), decreasing the temperature will favor the endothermic reaction, which is the reverse reaction. This will result in an increase in the concentration of B in the equilibrium mixture.

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  • 4. 

    In which reaction will be amount of product be increased by decreasing the pressure?

    • 2NO (g) + O2(aq) 2NO2 (g)

    • N2 (g) + 3H2 (g) 2NH3 (g)

    • 2NO2 (g) N2O4 (g)

    • CH4 (g) + H2O (g) CO (g) + 3H2 (g)

    Correct Answer
    A. CH4 (g) + H2O (g) CO (g) + 3H2 (g)
  • 5. 
    On 6 & 7.In the Haber Process, N2(g) + 3H2(g) <------>  2NH3(g) The following graph shows the effect of temperature and pressure on the yield.Which of the following options does not explain why the yield increases when temperature decreases? - ProProfs

    On 6 & 7.In the Haber Process, N2(g) + 3H2(g) <------>  2NH3(g) The following graph shows the effect of temperature and pressure on the yield.Which of the following options does not explain why the yield increases when temperature decreases?

    • The system responds in a way so as to counteract the decreased temperature.

    • The system favours the forward reaction which is exothermic.

    • The system favours the forward reaction which is endothermic.

    • The system responds in a way in accordance with Le Chatelier's principle, replacing the heat lost by raising the temperature.

    Correct Answer
    A. The system favours the forward reaction which is endothermic.
  • 6. 
    The equation show the equilibrium between silver ions and iron(II) ions.Ag+(aq) + Fe2+(aq) <----> Ag(s) + Fe3+(aq) Which one of the following statements is not true for the above equilibrium? - ProProfs

    The equation show the equilibrium between silver ions and iron(II) ions.Ag+(aq) + Fe2+(aq) <----> Ag(s) + Fe3+(aq) Which one of the following statements is not true for the above equilibrium?

    • At equilibrium, the rate of the forward reaction is equal to the rate of the backward reaction.

    • The concentration of all reactants and products are independent of the external pressure.

    • Addition of dilute hydrochloric acid to precipitate silver chloride would cause the equilibrium to shift to the left.

    • The yield of silver metal could be significantly increased by adding a catalyst.

    Correct Answer
    A. The yield of silver metal could be significantly increased by adding a catalyst.
  • 7. 

    Which of the following options does not explain why the yield increases when pressure is increased?

    • The volume of gas molecules decreases in the forward reaction.

    • The number of moles of gas molecules increases in the forward reaction.

    • An increase in pressure due to decreasing volume causes the reaction to shift to the side with the fewer moles of gas.

    • The position of equilibrium shifts to the right to favour the forward reaction.

    Correct Answer
    A. The number of moles of gas molecules increases in the forward reaction.
    Explanation
    An increase in pressure due to decreasing volume causes the reaction to shift to the side with the fewer moles of gas. This is because according to Le Chatelier's principle, when the pressure is increased, the system will try to decrease the pressure by shifting the equilibrium towards the side with fewer moles of gas. This explanation is supported by the fact that the volume of gas molecules decreasing in the forward reaction and the position of equilibrium shifting to the right to favor the forward reaction both contribute to an increase in yield when pressure is increased.

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  • Current Version
  • Mar 21, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • May 26, 2009
    Quiz Created by
    Vincenttan
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