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Chemistry Test 199
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Chemistry Test 199
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  • Question 1/10
    4 / -1

    A sample of HI (g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI (g) is 0.04 atm. What is Kp for the given equilibrium?

    Solutions

     

  • Question 2/10
    4 / -1

    An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and H2S gases in the flask. When the decomposition reaction reaches equilibrium the total pressure in the flask rises to 0.84 atm? The equilibrium constant for NH4HS decomposition at this temperature is:

    Solutions

     

  • Question 3/10
    4 / -1

    Which of the following conclusions is correct for a certain reaction whose Kc is 2 × 10−3 at 25°C and 2 × 10−2 at 50°C?

    Solutions

    The given data suggests an increase in the value of K with an increase in the temperature. This case is true for endothermic reactions. For such reactions, the enthalpy of products is more than the enthalpy of the reactants and thus the sign of ∆H will be positive.

     

  • Question 4/10
    4 / -1

    A reaction system in equilibrium according to reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) in one litre vessel at a given temperature was found to be 0.12 mole each of SO2 and SO3 and 5 mole of O2. In another vessel of one litre contains 32 g of SO2 at the same temperature. What mass of O2 must be added to this vessel to order that at equilibrium 20% of SO2 is oxidized to SO3?

    Solutions

     

  • Question 5/10
    4 / -1

    For a reaction at equilibrium, which of the following statements is correct?

    Solutions

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

     

  • Question 6/10
    4 / -1

    For the reaction, PCl3 (g)+Cl2 (g) ⇌ PCl5 (g) the position of equilibrium can be shifted to the right by

    Solutions

    PCl3 (g)+Cl2 (g) ⇌ PCl5 (g)

    According to Le-Chatelier's principle, on increasing the volume of a reactant, the reaction proceeds in the forward direction. Hence, on addition of Cl2 to above reaction, the equilibrium will shift to the right.

     

  • Question 7/10
    4 / -1

    Which of the following statements is correct?

    Solutions

    At equilibrium, the concentration of reactants and products may or may not become equal, but it becomes constant, i.e., there occurs no further change in the concentration of reactants and products.

    Also, the rate of the forward reaction is equal to the rate of backward reaction: rf = rb. This is the state of dynamic equilibrium.

    Equilibrium can be attained from both sides, whether we start from reactants or the products.

    While, if there is any formation of precipitate in the reaction, the reaction no longer remains in the state of equilibrium and the reaction becomes unidirectional.

     

  • Question 8/10
    4 / -1

    In a chemical reaction, the rate constant for the backward reaction is 7.5 × 10–4 and the equilibrium constant is 1.5. The rate constant for the forward reaction is -

    Solutions

    Apply the formula, K = Kf/Kb

    we get, Kf = 1.5 × 7.5 × 10−4 = 1.125 × 10−3

     

  • Question 9/10
    4 / -1

    At constant temperature, the equilibrium constant (Kp) for the decomposition reaction N2O4 ⇌ 2NO2 is expresses by  where P = pressure, x = extent of decomposition. Which one of the following statements is true?

    Solutions

    The reaction proceeds with an increase in volume.

    So, an increase in pressure (P) favours the reaction in the backward direction.

    Thus, Kp remains constant with change in P and x.

     

  • Question 10/10
    4 / -1

    For the reaction, CO(g) + Cl2(g) ⇌ COCl2(g), the value of Kp/Kc is equal to:

    Solutions

    Kp = Kc(RT)Δn

    Δn = Number of gaseous molecule of products − Number of gaseous molecules of reactants

    CO(g) + Cl2(g) → COCl2(g)

    ∴ Δn = 1 − 2 = −1

    ∴ Kp = Kc(RT)−1

     

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