List of top Chemistry Questions on Equilibrium Constant

For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the equilibrium constant Kc is 0.5 at 400 K. If [N₂] = 0.1 M, [H₂] = 0.2 M, and [NH₃] = 0.05 M, what is the reaction quotient Qc?

37.8 g \( N_2O_5 \) was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K: \[ 2N_2O_5(g) \rightarrow 2N_2O_4(g) + O_2(g) \]
The total pressure at equilibrium was found to be 18.65 bar. Then, \( K_p \) is: Given: \[ R = 0.082 \, \text{bar L mol}^{-1} \, \text{K}^{-1} \]

For the reaction \( \text{N}_2(g) + 3 \, \text{H_2(g) \rightleftharpoons 2 \, \text{NH}_3(g) \), the equilibrium constant \( K_c \) at a certain temperature is \( 0.5 \). If the initial concentrations of \( \text{N}_2 \), \( \text{H}_2 \), and \( \text{NH}_3 \) are \( 1.0 \, \text{mol/L} \), \( 1.0 \, \text{mol/L} \), and \( 0 \, \text{mol/L} \) respectively, calculate the equilibrium concentrations of all species.}
In which of the following equilibria, Kp and Ke are NOT equal?
At \(298\ K\)
\(N_2( g)+3H_2( g)⇌2NH_3( g),K_1=4×10^5\)
\(N_2( g)+O_2( g)⇌2NO(g),K_2=1.6×10^{12}\)
\(H_2( g)+1 2O_2( g)⇌H_2O(g),K_3=1.0×10^{−13}\)
Based on above equilibria, the equilibrium constant of the reaction, 
\(2NH_3( g)\)+\(\frac5 {2}\) \(O_2( g)⇌2NO(g)+3H_2O(g)\) is _______ \(×10^{−33 }\). (Nearest integer)
The equilibrium constant for the reaction
\(Zn(s)+Sn^{2+}(aq)⇌Zn^{2+}(aq)+Sn(s)\, is\, 1×10^{20}\) at \(298 K\). 
The magnitude of standard electrode potential of \(Sn/Sn^{2+}\) if \(E^{\degree}_{ Zn^{2+}/Zn}= –0.76V \) is _______ \(×10^{−2} V\). (Nearest integer).
(Given : \(\frac{2.303RT}{ F}\) \(=0.059 V \))
\(PCl_5\) dissociates as
\(PCl_5(g) ⇌ PCl_3(g)+ Cl_2(g)\)
\(5\) moles of \(PCl_5\) are placed in a \(200\) litre vessel which contains \(2\) moles of \(N_2\) and is maintained at \(600\ K\). The equilibrium pressure is \(2.46\) atm. The equilibrium constant Kp for the dissociation of \(PCl_5\) is ______ \(× 10^{–3}\). (nearest integer) 
(Given: \(R = 0.082\) L atm K–1 mol–1; Assume ideal gas behaviour)
At \(298\ K\), the equilibrium constant is \(2 × 10^{15}\) for the reaction:
\(Cu(s)+2Ag+(Aq)⇌Cu^{2+}(aq)+2Ag(s)\)
The equilibrium constant for the reaction:
\(\frac 12Cu^{2+}(aq)+Ag(s)+(Aq)⇌\frac 12Cu(s)+Ag^+(aq)\) is \(x \times10^{-8}\).
The value of \(x\) is ______ . (Nearest integer)
If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction ${Zn(s) + cu^{2+} (aq) <=> Zn^{2+} (aq) + Cu(s)}$ at 300 K is approximately. ${(R = 8 \; JK^{-1} \; mol^{-1} , F = 96000 \; C \; mol^{-1})}$