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Chemical Equilibrium Test - 12
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Chemical Equilibrium Test - 12
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  • Question 1/10
    1 / -0

    If Kp​ for a reaction, A(g)+2B(g) ⇌ 3C(g) + D(g) is 0.05 atm at 1000K, its Kc​ in terms of R will be:

    Solutions

     For the reaction A(g) + 2B(g) ⇌ 3C(g) + D(g)

    Δn = 3 + 1 − (1+2) = 1

    Kp​ = Kc​(RT)Δn

    0.05 = Kc​ × (R×1000)1

     

  • Question 2/10
    1 / -0

    The vapour density of N2​O4​ at a certain temperature is 30. What is the percentage dissociation of N2​O​4 at this temperature ?

    Solutions

     

  • Question 3/10
    1 / -0

    If PCl5 is 80% dissociated at 523 K, what is the vapour density of the equilibrium mixture at 523 K ?

    Solutions

    The correct option is A 57.92
    PCl5(s) ⇌ PCl3(g) + Cl2(g)
    n = 2
    α = 80% = 80/100 = 0.8
    theoretical vapour/Normal vapour density,

    D = Normal molar mass/2 = 208.5/2 = 104.25

    vapour density of the equilibrium mixture, d=?
    we have the relation

     

  • Question 4/10
    1 / -0

    Ammonium carbamate when heated to 2000C gives a mixture of NH3 and CO2 with vapour density of 13.

    The degree of dissociation of ammonium carbonate is:

    Solutions

     

  • Question 5/10
    1 / -0

    In the reaction, H2​(g)+I2​(g) ⇌ 2HI(g) the concentration of H2​, I2​ and HI at equilibrium are 8.0, 3.0 and 28 moles per litre respectively. What will be the equilibrium constant ?

    Solutions

    H2​(g)+I2​(g)⇌2HI(g)

    Applying law of mass action,

    Given : [H2​]=8.0 mol L−1, [I2​]=3.0 mol L−1 ,[HI]=28.0 mol L−I

     

  • Question 6/10
    1 / -0

    For the reaction, N2(g) + 3H2(g) ⇌ 2NH3(g), the partial pressures of N2 and H2 are 0.80 and 0.40 atmosphere respectively at equilibrium. The total pressure of the system is 2.80 atmosphere. What is Kp for the above reaction?

    Solutions

     

  • Question 7/10
    1 / -0

    A two litre flask contains 1.4 gm nitrogen and 1.0 gm hydrogen. The ratio of active mass of nitrogen and hydrogen would be -

    Solutions

     

  • Question 8/10
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    The reaction A(g)+B(g) ⇋ C(g)+D(g) is studied in a one litre vessel at 250∘C. The initial concentration of A was 3n and that of B was n. When equilibrium was attained, equilibrium concentration of C was found to be equal to the equilibrium concentration of B. What is the concentration of D at equilibrium?

    Solutions

     

  • Question 9/10
    1 / -0

    The value of Kc​ for the reaction :

    A + 3 B ⇌ ​2C at 400°C is 0.5. Calculate the value of KP​

    Solutions

     

  • Question 10/10
    1 / -0

    Two moles of ammonia was introduced in an evacuated vessel of 1L capacity. At high temperature, the gas undergoes partial dissociation according to the equation:

    2NH3​(g) ⇌ N2​(g) + 3H2​(g)

    At equilibrium the concentration of ammonia was found to be 1mol. What is the value of K ?

    Solutions

    Hence we have :

    At equilibrium : [NH3​] = 2−2α = 1 or α = 1/2

     

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