For the following equilibrium, K_c= 6.3 × 10¹⁴ at 1000 K

$\mathrm{NO}\left(\mathrm{g}\right)$ $+$ ${\mathrm{O}}_3$ $\left(\mathrm{g}\right)$ $\to$ ${\mathrm{NO}}_2\left(\mathrm{g}\right)$ $+$ ${\mathrm{O}}_2$ $\left(\mathrm{g}\right)$ $$

The value of K_c for the reverse reaction is:

$1.$ $2.33$ $\times$ ${10}^{-16}$
$2.$ $1.59$ $\times$ ${10}^{-15}$
$3.$ $2.67$ $\times$ ${10}^{-13}$
$4.$ $4.47$ $\times$ ${10}^{14}$

\(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{NH}_3\right]^4\left[\mathrm{O}_2\right]^5}{[\mathrm{NO}]^4\left[\mathrm{H}_2 \mathrm{O}]^6\right.}\)
The balanced chemical equation corresponding to the above-mentioned expression is:

One mole of H₂O and one mole of CO are taken in a 10 L vessel and heated to
725 K. At equilibrium, 40% of water(by mass) reacts with CO according to the equation,

H₂O _(g) + CO _(g)  $\leftrightharpoons$H_2 (g) + CO_2 (g)

The equilibrium constant for the above-mentioned reaction would be:

The equilibrium pressure of C₂H₆ when it is placed in a flask at 4.0 atm pressure at  899 K would be:

C₂H_6 (g)  $\leftrightharpoons$ C₂H_4 (g) + H_2 (g)

( K_p = 0.04 atm at 899 K)

A sample of pure PCl₅ was introduced into an evacuated vessel at 473 K.
After equilibrium was attained, a concentration of PCl₅ 
was found to be 0.5 × 10^–1 mol L^–1. If the value of
 K_c is 8.3 × 10^–3 mol L^–1, the concentrations of
PCl₃ and Cl₂ at equilibrium would be:

PCl_5 (g)  $\leftrightharpoons$PCl_3 (g) + Cl_2(g)
 

For the reaction, 2NOCl (g) $\rightleftharpoons$ 2NO (g) + Cl₂ (g); K_p= 1.8 × 10^–2 atm at 500 K.

The value of K_c for above mentioned reaction would be:

$1.$ $4.33$ $\times$ ${10}^{-4}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$2.$ $4.33$ $\times$ ${10}^4$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$3.$ $1.65$ $\times$ ${10}^{-5}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$4.$ $2.39$ $\times$ ${10}^{-3}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$$

 At 450 K, K_p= 2.0 × 10¹⁰ bar^-1 for the given reaction at equilibrium

$2{{\mathrm{SO}}_2}_{(\mathrm{g}) }+$ ${{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}$ $\rightleftharpoons$ $2{{\mathrm{SO}}_3}_{\left(\mathrm{g}\right)}$ $$

The value of  K_c at this temperature would be :

$1.$ $7.48$ $\times {10}^{12}$ ${\mathrm{M}}^{-1}$
$2.$ $6.56$ $\times$ ${10}^{11}$ ${\mathrm{M}}^{-1}$
$3.$ $7.48$ $\times$ ${10}^{11}$ ${\mathrm{M}}^{-1}$
$4.$ $1.23$ $\times$ ${10}^{10}$ ${\mathrm{M}}^{-1}$

For the reaction: ${\mathrm{FeO}}_{\left(\mathrm{s}\right)}$ $+$ ${\mathrm{CO}}_{\left(\mathrm{g}\right)}$ $\rightleftharpoons$ ${\mathrm{Fe}}_{\left(\mathrm{s}\right)}$ $\hspace{0.17em}+\hspace{0.17em}{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)},$ ${\mathrm{K}}_{\mathrm{p}}$ $=$ $0.265$  at 1050 K. If the initial partial pressures are p_CO= 1.4 atm and ${\mathrm{p}}_{{\mathrm{CO}}_2}$= 0.80 atm, the partial pressure of CO₂ at equilibrium at 1050 K would be:

For the reaction, 

${\mathrm{N}}_2$ $\left(\mathrm{g}\right)$ $+$ $3{\mathrm{H}}_2\left(\mathrm{g}\right)$ $\rightleftharpoons$ $2{\mathrm{NH}}_3$ $\left(\mathrm{g}\right);$ $$
${\mathrm{K}}_{\mathrm{c}}=$ $0.061$ ${\mathrm{mol}}_{}^{-2}{\mathrm{L}}^2$  at 500K. At a particular instant of time, [N₂] = 3.0 mol L^–1, [H₂] = 2.0 mol L^–1  and [NH₃] = 0.5 mol L^–1 .

True statement among the following is: 

1. Reaction is at equilibrium.

2. Reaction will proceed in the forward direction.

3. Reaction will proceed in the backward direction.

4. Can't predict the direction of the reaction.
 

At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO₂ in equilibrium with solid carbon has 90.55% CO by mass. 

${\mathrm{C}}_{\left(\mathrm{s}\right)}$ $+$ ${{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$ $\rightleftharpoons 2{\mathrm{CO}}_{\left(\mathrm{g}\right)}$

At the specified temperature, K_c for this reaction would be

$1.$ $0.25$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$2.$ $0.34$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$3.$ $0.15$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$4.$ $1.25$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$