Effect on Kc

Q. Equilibrium constant, $K_C$ for the reaction
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ at $500K$ is $0.061$
At a particular time, the analysis shows that composition of the reaction mixture is $3.0mol{L}^{-1}{N}_2,2.0mol{L}^{-1}{H}_2$ and $0.5mol{L}^{-1}N{H}_3.$ Is the reaction at equilibirium and if not in which direction does the reaction tend to proceed to reach equilibrium?

1. at equilibrium
2. not at equilibrium, backwards shift
3. not at equilibrium, forward shift
4. can not be predicted

Q.

Does a catalyst change the equilibrium constant?

Q. What will be the effect of addition of a catalyst at constant temperature?

1. The equilibrium constant will remain constant
2. $\Delta \text{H}$ of the reaction will remain constant
3. $k_f$ and $k_b$ will increase by the same extent
4. Equilibrium composition will change

Q. Given the reaction between $2$ gases represented by $A_2$ and $B_2$ to give the compound $AB\left(g\right)$.
$A_2\left(g\right)+B_2\left(g\right)\rightleftharpoons 2AB\left(g\right)$
At equilibrium, the concentration of:
$A_2=3.0\times {10}^{-3}\text{M}$
$B_2=4.2\times {10}^{-3}\text{M}$
$AB=2.8\times {10}^{-3}\text{M}$
If the reaction takes place in a sealed vessel at $527{}^{\circ }\text{C}$, then the value of $K_c$ will be:

1. $2.0$
2. $1.9$
3. $0.62$
4. $4.5$

Q. For the reaction $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right),K_c=47.6$, If the initial number of moles of each reactant and product is 1 mole, then in equilibrium:

1. $\left[I_2\right]=\left[H_2\right];\left[I_2\right]>\left[HI\right]$
2. $\left[I_2\right]<\left[H_2\right];\left[I_2\right]=\left[HI\right]$
3. $\left[I_2\right]=\left[H_2\right];\left[I_2\right]<\left[HI\right]$
4. $\left[I_2\right]>\left[H_2\right];\left[I_2\right]=\left[HI\right]$

Q. Equilibrium constant, $K_C$ for the reaction
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ at $500K$ is $0.061$
At a particular time, the analysis shows that composition of the reaction mixture is $3.0mol{L}^{-1}{N}_2,2.0mol{L}^{-1}{H}_2$ and $0.5mol{L}^{-1}N{H}_3.$ Is the reaction at equilibirium and if not in which direction does the reaction tend to proceed to reach equilibrium?

1. at equilibrium
2. not at equilibrium, backwards shift
3. not at equilibrium, forward shift
4. can not be predicted

Q. $A\left(g\right)+3B\left(g\right)\rightleftharpoons 4C\left(g\right)$
Initial concentration of A is equal to that of B. The equilibrium concentration of A and C are equal. $K_c$ of the reaction will be:

1. $0.08$
2. $0.8$
3. $8$
4. $80$

Q. In hte following reaction
$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
the equilibrium is not attained. The rate of forward reaction is greater than that of backward reaction. Thus, which of the following is the correct relation between $K_p$ and $Q_p$?

1. $K_p=Q_p$
2. $Q_p>K_p$
3. $Q_p<K_p$
4. $K_p=Q_p=1$

Q. The reaction quotient (Q) for a reaction is given as $Q=\frac{[N{H}_3{]}^2}{\left[N_2\right][H_2{]}^3}$ . The reaction will proceed from left to right if ........

1. $Q=0$
2. $Q>k_c$
3. $Q<k_c$
4. $Q=k_c$

Q. The $E_{\text{cell}}^0$ for the given cell reaction is $-0.32\text{V}$ at ${25}^{\circ }\text{C}$.
$Fe\left(s\right)+Z{n}^{2+}\left(aq\right)\rightleftharpoons Zn\left(s\right)+F{e}^{2+}\left(aq\right)$
What will be the value of $\log \left[F{e}^{2+}\right]$ at equilibrium when a piece of iron is placed in a $1\text{M}$ of $Z{n}^{2+}$ solution?

Q. In hte following reaction
$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
the equilibrium is not attained. The rate of forward reaction is greater than that of backward reaction. Thus, which of the following is the correct relation between $K_p$ and $Q_p$?

1. $K_p=Q_p$
2. $Q_p>K_p$
3. $Q_p<K_p$
4. $K_p=Q_p=1$