Effective Equilibrium Constant

Q. If the equilibrium constant for $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$ is $K$, the equilibrium constant for
$\frac{1}{2}{N}_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\rightleftharpoons NO\left(g\right)$
will be :

<!--td {border: 1px solid #cccccc;}br {mso-data-placement:same-cell;}--> Re-AIPMT 2015

1. $K^2$
2. $K$
3. $\frac{1}{2}K$
4. $\sqrt{K}$

Q.

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are

$NO\left(g\right)+0.5O_2\left(g\right)\underrightarrow{}{K}_{1}N{O}_2\left(g\right)$ and
$2N{O}_2\left(g\right)\underrightarrow{}{K}_{2}2NO\left(g\right)+O_2\left(g\right)$

1. K₂ = 1/K­₁

2. K₂ = K­₁²

3. K₂ = (K­₁)/2

4. K₂ = 1/K­₁²

Q. For the reaction, $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$, the equilibrium constant is $K_1$. The equilibrium constant is $K_2$ for $2NO\left(g\right)+O_2\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$. What is K for the reaction $N{O}_2\left(g\right)\rightleftharpoons \frac{1}{2}{N}_2\left(g\right)+O_2\left(g\right)$?

1. 
2. 
3. 
4. 

Q. The equilibrium constants of the following are
$N_2+3H_2\rightleftharpoons 2N{H}_3;K_1$
$N_2+O_2\rightleftharpoons 2NO;K_2$

$H_2+\frac{1}{2}{O}_2\rightleftharpoons H_{2}O;K_3$
The equilibrium constant (K) of the reaction:
$2N{H}_3+\frac{5}{2}{O}_2\stackrel{K}{\rightleftharpoons }2NO+3H_{2}O$ will be

1. $K_2{K}_3/K_1$
2. $K_2^3{K}_3/K_1$
3. $K_1{K}_3^3/K_2$
4. $K_2{K}_3^3/K_1$

Q.

Consider the following equilibria at ${25}^{\circ }C,2N{O}_{\left(g\right)}\rightleftharpoons N_{2\left(g\right)}+O_{2\left(g\right)};K_1=4\times {10}^{30}andN{O}_{\left(g\right)}+\frac{1}{2}B{r}_{2\left(g\right)}\rightleftharpoons NOB{r}_{\left(g\right)};K_2=1.4mo{l}^{-\frac{1}{2}}{L}^{\frac{1}{2}}.$ The value of K_C for the reaction (at same temperature) $\frac{1}{2}{N}_{2\left(g\right)}+\frac{1}{2}{O}_{2\left(g\right)}+\frac{1}{2}B{r}_{2\left(g\right)}\rightleftharpoons NOB{r}_{\left(g\right)}$ is :

1. $3.5\times {10}^{-31}$

2. $2.8\times {10}^{15}$

3. $5.6\times {10}^{30}$

4. $7.0\times {10}^{-16}$

Q.

A hypothetical reaction : $A_{\left(g\right)}+B_{\left(g\right)}\rightleftharpoons C_{\left(g\right)}+D_{\left(g\right)}$ occurs in a single step, the specific rate constant of forward reaction at TK is $2.0\times {10}^{-3}mo{l}^{-1}L{s}^{-1}$. When start is made with equimolar amounts of A and B, it is found that the concentration of A is twice that of C at equilibrium. The specific rate constant of the backward reaction is ?

1. $8.0\times {10}^{-3}mo{l}^{-1}L{s}^{-1}$

2. $1.5\times {10}^{2}mo{l}^{-1}L{s}^{-1}$

3. $Noneofthese$

4. $5.0\times {10}^{-4}mo{l}^{-1}L{s}^{-1}$

Q.

At certain temperature, a compound $A{B}_2$ dissociates as: $2A{B}_{2\left(g\right)}\to 2A{B}_{\left(g\right)}+B_{2\left(g\right)}$ with a degree of dissociation $\alpha$, which is very small compared to unity. The expression of $K_p$ in terms of $\alpha$ and total pressure P is ?

1. $\frac{{\alpha }^{2}P}{2}$

2. $\frac{{\alpha }^{2}P}{3}$

3. $\frac{{\alpha }^{3}P}{3}$

4. $\frac{{\alpha }^{3}P}{2}$

Q. The approach of the following equilibrium was observed kinetically from both directions
$PtC{l}_4^{2-}+H_{2}O\rightleftharpoons Pt\left(H_{2}O\right)C{l}_3^{-}+C{l}^{-}$
At 25°C, it is found $\frac{–d\left[PtC{l}_4^{2-}\right]}{dt}=(3.9\times {10}^{-5}{s}^{-1)})\left[PtC{l}_4^{2-}\right]-(2.1\times {10}^{-3}Lmo{l}^{-1}{s}^{-1})\left[Pt\right(H_{2}O\left)C{l}_3^{-}\right]\left[C{l}^{-}\right]$
Value of $K_C$ when fourth $C{l}^{-}$ is complexed in the reaction is:

1. $1.85\times {10}^{-2}$
2. $1.86\times 2$
3. $53.85$
4. $8.19\times {10}^{-8}$

Q. The equilibrium constants for the following are:
$N_2+3H_2\rightleftharpoons 2N{H}_3{K}_1$
$N_2+O_2\rightleftharpoons 2NO{K}_2$
$H_2+\frac{1}{2}{O}_2\to H_{2}O{K}_3$
The equilibrium constant (K) of the reaction:
$2N{H}_3+\frac{5}{2}{O}_2\stackrel{K}{\rightleftharpoons }2NO+3H_{2}O,$ will be

1. $K_1{K}_3^3/K_2$
2. $K_2{K}_3^3/K_1$
3. $K_2{K}_3/K_1$
4. $K_2^3{K}_3/K_1$

Q. If the equilibrium constant for
$N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$ is $K$, the equilibrium constant for $\frac{1}{2}{N}_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\rightleftharpoons NO\left(g\right)$ will be :-

1. $K$
2. $K^2$
3. $K^{1/2}$
4. $\frac{1}{2}K$