NEET Chemistry Chemical Equilibrium Kc&Kp MCQs

For the reversible reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ at a certain temperature, the partial pressures at equilibrium are $P_{SO_2} = 0.2$ atm, $P_{O_2} = 0.1$ atm, and $P_{SO_3} = 0.8$ atm. If the total pressure is suddenly doubled by adding an inert gas at constant volume, the new partial pressure of $SO_3$ at the newly established equilibrium will be closest to:

At 700 K, the equilibrium constant $K_p$ for the reaction $2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g)$ is $1.8 imes 10^{-6}$ atm. If 0.5 atm of $H_2S$ is introduced into an evacuated vessel at 700 K, what is the equilibrium partial pressure of $H_2$?

For the reaction $N_2O_4(g) \rightleftharpoons 2NO_2(g)$, $K_c = 4.6 imes 10^{-3}$ at 25°C. If 1 mole of $N_2O_4$ is placed in a 10 L container at 25°C, what is the approximate equilibrium concentration of $NO_2$?

The equilibrium constant $K_p$ for the reaction $A(g) + 2B(g) \rightleftharpoons C(g)$ is 0.25 at a certain temperature. If the initial partial pressures of A and B are 1 atm and 2 atm respectively, what is the equilibrium partial pressure of C?

For the reaction $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$, at a given temperature, $K_p = 1.8$. At equilibrium, the partial pressure of $PCl_5$ is 0.2 atm. If the total pressure is 2 atm, what is the partial pressure of $Cl_2$?

A reaction has $\Delta n_g = -1$ and $K_p = 2$ atm$^{-1}$ at 298 K. What is the value of $K_c$ for this reaction at 298 K? (R = 0.0821 L atm mol$^{-1}$ K$^{-1}$)

For the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, if the concentrations of $N_2$, $H_2$, and $NH_3$ are 1 M, 3 M, and 2 M respectively at equilibrium, what is the value of $K_c$?

Which of the following is true about $K_c$ and $K_p$ for the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$?

The unit of $K_c$ for the reaction $A(g) + B(g) \rightleftharpoons C(g)$ is:

For a reaction with $K_c = 1$, at equilibrium: