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One mole of nitrogen is mixed with three...

One mole of nitrogen is mixed with three moles of hydrogen in a 4 litre container. If 0.25 per cent of nitrogen is converted into ammonia by the following reaction
` N_2(g) +3H_2 hArr 2NH_3(g)`
calculate the equilibrium constant of the reaction in concentration units. What will be the value of K for the following reaction?
` (1)/(2) N_2 (g) + (3)/(2) H_2 hArr NH_3 (g)`

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The correct Answer is:
A, C
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Knowledge Check

  • In the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) the value of the equilibrium constant depends on

    A
    volume of the reaction vessel
    B
    total pressure of the system
    C
    the initial concentration of nitrogen and hydrogen
    D
    the temperature

  • For the reversible reaction N_2(g) +3H_2(g) hArr 2NH_3(g) +"Heat" The equilibrium shifts in forward directions.

    A
    by increasing the concentration of `NH_3 (g)`
    B
    by decreasing the pressure
    C
    by decreasing the concentration of `N_2(g) and H_2(g)`
    D
    by increasing pressure and decreasing temperature

  • For the reaction, N_2[g] + 3H_2[g] hArr 2NH_3[g] , Delta H = …

    A
    `DeltaU - 2RT`
    B
    `DeltaU + 2RT`
    C
    `DeltaU + RT`
    D
    `DeltaU - RT`.

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