The equilibrium constant, K for the reaction: 

$2HI\left(g\right)$ $H_2\left(g\right) + I_2\left(g\right)$ at room temperature is 2.85 and at 698K is $1.4$ $\times {10}^{-2}$. This implies that the forward reaction is

(1) Exothermic

(2) Endothermic

(3) Neither exothermic nor endothermic

(4) Unpredictable

Which of the following reactions is favoured by increased of temperature?

1. $N_2+H_2\rightleftharpoons 2N{H}_3+22.9<mspace\; width="1em"></mspace>kcl$

2. $N_2\left(g\right)<mspace\; width="1em"></mspace>+O_2\rightleftharpoons 2NO\left(g\right)<mspace\; width="1em"></mspace>-42.9<mspace\; width="1em"></mspace>kcl<mspace\; width="1em"></mspace>$

3. $2SO\left(g\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>O_2\left(g\right)<mspace\; width="1em"></mspace>\rightleftharpoons 2S{O}_3\left(g\right)<mspace\; width="1em"></mspace>+45.3kcl$

4. $H_2\left(g\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>C{l}_2\left(g\right)<mspace\; width="1em"></mspace>-<mspace\; width="1em"></mspace>44.0kcl<mspace\; width="1em"></mspace>\rightleftharpoons 2HCl<mspace\; width="1em"></mspace>\left(g\right)<mspace\; width="1em"></mspace>$

One mole of N${}_2$ is mixed 3 moles of H${}_2$ in one litre container. If 50% of N${}_2$ is converted into ammonia by the reaction N${}_2$(g) + 3H₂ (g) $\rightleftharpoons$  2NH${}_3$(g), then the total number of moles of gas at the equilibrium are 

1. 1.5

2. 4.5 

3. 3.0 

4. 6.0

The decomposition of N${}_2$O${}_4$ to is carried out at 280$°$C in chloroform. When equilibrium is reached, 0.2 mol N${}_2$O${}_4$ and 2 $\times$10${}^{-3}$ mol of NO${}_2$ are present in 2L solution. The equilibrium constant for the reaction N${}_2$O${}_4$ $\rightleftharpoons$ 2NO${}_2$is 

1. 1$\times$10${}^{-2}$

2. 2$\times$10${}^{-3}$

3. 1$\times$10${}^{-5}$

4. 2$\times$10${}^{-5}$

For the follwing gaseous equilibria X,Y and Z at 300K 

X : 2SO${}_2$$+O_2\rightleftharpoons 2S{O}_3$

Y : $PC{I}_5\rightleftharpoons PC{I}_3+C{I}_2$

Z : 2HI $\rightleftharpoons$ H${}_2$ + I${}_2$

Ratio of K${}_p$ and K${}_c$ in the increasing order is: 

1. X=Y=Z

2. X<Y<Z

3. X<Z<Y

4. Z<Y<X

$N_2+<mspace\; width="1em"></mspace>3H_2\rightleftharpoons 2N{H}_3$
1 mole \(N_2\) and \(3H_2\) are at 4 atm.
Equilibrium pressure is found to be 3 atm. find the \(K_p\)

1. \(\frac{1}{0.5(1.5)^3}\) 

2. \(\frac{1}{0.5(0.5)^3}\) 

3. \(\frac{3\times3}{0.5(0.5)^3}\) 

4. None of these 

4 moles of A are mixed with 4 moles of B,

when 2 moles of C are formed at equilibrium

according to the reaction A +B $\rightleftharpoons$C+ D 

The value of the equilibrium constant is: 

1. 4

2. 1

3. 1/2

4. 1/4

Which of the following can act as Lowry-Bronsted acid as well as a base ?

1. CI${}^{-}$

2. HCO${}_3^{-}$

3. H${}_3$O+

4. SO${}_4^{2-}$

In the reaction HCN + H${}_2$O $\rightleftharpoons <mspace\; width="1em"></mspace>H_3{O}^{+}+<mspace\; width="1em"></mspace>C{N}^{-}$ the conjugate acid- base pair is 

1. HCN,H${}_3$O${}^{+}$

2. HCN,CN${}^{-}$

3. $H_{2}O,<mspace\; width="1em"></mspace>C{N}^{-}$

4. $C{N}^{-},H_3{O}^{+}$

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) $\stackrel{}{\rightleftharpoons }$ CO₂(g)+ NO(g)One mole of each of the four gas is mixed in one litre container and the reaction is allowed to reach equilibrium state. When excess of baryta water (Ba(OH)₂) is added to the equilibrium mixture, the weight of white ppt (BaCO₃) obtained is 236.4 gm. The equilibrium constant K_c of the reaction is (Ba = 137)

(1) 1.2

(2) 2.25

(3) 2.1

(4) 3.6