Law of chemical equilibrium, Kp and Kc

For the reaction \(\mathrm{A(g) \rightleftharpoons 2B(g)}\), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K.

[Given : R = 0.0831 L atm \(\mathrm{mol^{-1}\,K^{-1}}\)]

\(K_p\) for the reaction at 1000 K is

For the reaction \(2A \rightleftharpoons B + C\), \(K_c = 4\times10^{-3}\). At a given time, the composition of reaction mixture is : \([A]=[B]=[C]=2\times10^{-3}\) M.

Then, which of the following is correct?

In which of the following equilibria, \(K_p\) and \(K_c\) are NOT equal?

Consider the following reaction in a sealed vessel at equilibrium with concentrations of \(N_2 = 3.0\times10^{-3}\) M, \(O_2 = 4.2\times10^{-3}\) M and \(NO = 2.8\times10^{-3}\) M.

\(2NO_{(g)} \rightleftharpoons N_{2(g)} + O_{2(g)}\)

If 0.1 mol \(L^{-1}\) of \(NO_{(g)}\) is taken in a closed vessel, what will be degree of dissociation (\(\alpha\)) of \(NO_{(g)}\) at equilibrium?

\(3O_2(g) \rightleftharpoons 2O_3(g)\)

for the above reaction at 298 K, \(K_c\) is found to be \(3.0 \times 10^{-59}\). If the concentration of \(O_2\) at equilibrium is 0.040 M then concentration of \(O_3\) in M is

The equilibrium constants of the following are :

\(N_2 + 3H_2 \rightleftharpoons 2NH_3\) \(K_1\)

\(N_2 + O_2 \rightleftharpoons 2NO\) \(K_2\)

\(H_2 + \frac{1}{2}O_2 \rightarrow H_2O\) \(K_3\)

The equilibrium constant (K) of the reaction : \(2NH_3 + \frac{5}{2}O_2 \overset{K}{\rightleftharpoons} 2NO + 3H_2O\), will be :

Which one of the following statements is not correct ?

A 20 litre container at 400 K contains \(CO_2\)(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of \(CO_2\) attains its maximum value, will be :

(Given that : \(SrCO_3(s) \rightleftharpoons SrO(s) + CO_2(g)\), \(K_p = 1.6\) atm)