Characteristics of Equilibrium Constant

Q. In a chemical reaction, $A+2B\stackrel{K}{\rightleftharpoons }2C+D$, the initial concentration of B was 1.5 times of the concentration of A, but the equilibrium concentrations of A and B were found to be equal. The equilibrium constant (K) for the aforesaid chemical reaction is:

1. 3
2. 1
3. 4
4. 2

Q.

For the reaction $H_2$ (g) + $I_2$ (g) $\leftrightharpoons$ 2HI(g)the equilibrium constant $K_p$ changes with

1. catalyst

2. Total pressure

3. the amounts of and present

4. temperature

Q.

The equilibrium constant in a reversible reaction at a given temperature

1. Depends on the initial concentration of the reactants

2. Does not depend on the initial concentrations

3. Depends on the concentration of the products at equilibrium

4. It is not characteristic of the reaction

Q. Pure ammonia is placed in a vessel at a temperature where its dissociation is appreciable. At equilibrium,

1. K_p does not change significantly with pressure
2. α does not change with pressure
3. concentration of NH₃ does not change with pressure
4. concentration of H₂ is less than that of N₂

Q.

For the homogeneous gas phase equilibrium $4N{H}_3\left(g\right)+5O_2\left(g\right)\iff 4NO\left(g\right)+6H_{2}O\left(g\right)$ the units of equilibrium constant ${}^{\prime }{K}_C^{\prime }$ are

1. mol L${}^{-1}$

2. L mol${}^{-1}$

3. mol${}^2$ L${}^2$

4. L${}^2$ mol${}^{-2}$

Q. For the chemical equilibrium, $CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right),△H^o,$ can be determined from which one of the following plots

1. 
2. 
3. 
4. 

Q.

At the equilibrium of the reaction :
$A_{\left(g\right)}+2B_{\left(s\right)}\rightleftharpoons C_s+2D_{\left(s\right)}+E_{\left(g\right)},$ A reacts to the extent of 20% at 400 K and to the extent of 25% at 300K. The equilibrium shifts in forward direction

1. On increasing both pressure and temperature

2. On decreasing both pressure and temperature

3. On decreasing temperature only

4. On using the catalyst

Q. Consider the general hypothetical reaction:
$A\left(s\right)\leftrightharpoons 2B\left(g\right)+3C\left(g\right)$
If the concentration of C at equilibrium is doubled, then after the equilibrium is re-established, the concentration of B will be :

1. Twice of its original value
2. Half of its original value
3. $2\sqrt{2}$ times of original value
4. $\frac{1}{2\surd 2}$ times the original value

Q. In an alkaline solution, the following equilibria exist.
$S^{2-}+S\to S_2^{2-}$equilibrium constant $K_1$
$S_2^{2-}+S\to S_3^{2-}$ equilibrium constant $K_2$
$K_1$ and $K_2$ have the values 12 and 11, respectively.
$S_3^{2-}\to S^{2-}+2S$. What is equilibrium constant for the reaction?

1. $132$
2. $0.198$
3. $7.58\times {10}^{-3}$
4. $1.09$

Q. Match the following.
$\begin{array}{cc}\text{Reaction}& \text{Degree of dissociation in terms of}\\ \text{(Homogeneous gaseous phase)}& \text{equilibrium constant}\\ \text{(a)}A\left(g\right)+B\left(g\right)\rightleftharpoons 2C\left(g\right)& \text{(p)}\left(\sqrt{K}\right)/(1+\sqrt{K})\\ \text{(b)}2A\left(g\right)\rightleftharpoons B\left(g\right)+C\left(g\right)& \text{(q)}\left(\sqrt{K}\right)/(2+\sqrt{K})\\ \text{(c)}A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right)+D\left(g\right)& \text{(r)}2K/(1+2K)\\ \text{(d)}AB\left(g\right)\rightleftharpoons \frac{A}{2}\left(g\right)+\frac{B}{2}\left(g\right)& \text{(s)}\frac{2\sqrt{K}}{1+2\sqrt{K}}\\ & \text{(t) K}\end{array}$

1. $\text{a}–\text{q},\text{b}–\text{s},\text{c}-\text{p},\text{d}-\text{r}$
2. $\text{a}–\text{q},\text{b}–\text{p},\text{c}-\text{s},\text{d}-\text{r}$
3. $\text{a}–\text{r},\text{b}–\text{s},\text{c}-\text{p},\text{d}-\text{q}$
4. $\text{a}–\text{s},\text{b}–\text{p},\text{c}-\text{r},\text{d}-\text{q}$