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The following equilibrium constnats are ...

The following equilibrium constnats are given:
`N_(2)+3H_(2)hArr2NH_(3),K_(1)`
`N_(2)+O_(2)hArr2NO,K_(2)`
`H_(2)+1/2O_(2)hArrH_(2)O,K_(3)`
The equilibrium constant for the oxidation of 2 mol of `NH_(3)` to give NO is

A

`K_(1) . (K_(2))/(K_(3))`

B

`K_(2). (K_(3)^(3))/(K_(1))`

C

`K_(2) . (K_(3)^(2))/(K_(1))`

D

`K_(2)^(2) (K_(3))/(K_(1))`

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The equilibrium constants of the following are - N_(2) + 3H_(2) hArr 2 NH_(3) , K_(1) " " N_(2) + O_(2) hArr 2 NO , K_(2) H_(2) + (1)/(2) O_(2) to H_(2)O , K_(3) The equilibrium constant (K) of the reaction : 2NH_(3) + (5)/(2) O_(2) overset(K)(hArr) 2 NO + 3 H_(2) O , will be -

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Knowledge Check

  • Given : N_2(g) + 3H_2(g) iff 2NH_3(g), K_1 N_2(g) + O_2(g) iff 2NO(g), K_2 H_2(g) + 1/2 O_2(g) iff H_2O(g), K_3 The equilibrium constant for, 2NH_3(g) + 5/2 O_2(g) iff 2NO(g) + 3H_2O(g) will be :

    A
    `K_1K_2K_3`
    B
    `(K_1K_2)/K_3`
    C
    `(K_1K_3^2)/K_2`
    D
    `(K_2K_3^3)/K_1`

  • The equilibrium constant for the reactions - (i) N_2+3H_2iff2NH_3 (ii) N_2+O_2iff2NO and (iii) H_2+1/2O_2iffH_2O are K_1, K_2 and K_3 respectively. The equilibrium constant of the reaction 2NH_3+5/2O_2iff2NO+3H_2O in terms of K_1 , K_2 and K_3 is

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    `K_1K_2/K_3`
    B
    `(K_1K_3^2)/K_2`
    C
    `(K_2K_3^3)/K_1`
    D
    `K_1K_2K_3`

  • Consider the following gaseous equilibria given below: N_2 + 3H_2 iff 2NH_3 , Eqm. Constant = K_1 N_2 + O_2 iff 2NO , Eqm. Constant = K_2 H_2 + 1/2O_2 iff H_2O , Eqm. Constant = K_3 The equilibrium constant for the reaction, 2NH_3 + 5/2 O_2 iff 2NO + 3H_2O in terms of K_1, K_2 and K_3 will be :

    A
    `K_1K_2K_3`
    B
    `(K_1K_2)/K_3`
    C
    `(K_1K_3^2)/K_2`
    D
    `(K_2K_3^3)/K_1`

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