At 1990 K and 1 atm pressure, there are an equal number of Cl₂ molecules and Cl atoms in the reaction mixture.
The value of K_P for the reaction ${\mathrm{Cl}}_{2\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{Cl}}_{\left(\mathrm{g}\right)}$ under the above conditions is x × 10^–1. The value of x is:

1. 4

2. 8

3. 5

4. 10

For the reaction A_(g)$\to$(B)_(g), the value of the equilibrium constant at 300 K and 1 atm is equal to 100.0. The value of $∆$_rG for the reaction at 300 K and 1 atm in J mol^–1 is – xR, where x is:
(R = 8.31 J mol^–1 K^–1 and ln 10 = 2.3)

1. 1400

2. 1380

3. 1360

4. 1340

For a reaction; $X<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>Y<mspace\; width="1em"></mspace>\leftrightharpoons <mspace\; width="1em"></mspace>2Z$, 1.0 mol of X, 1.5 mol of Y and 0.5 mol of Z were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of Z was 1.0 mol L^–1 . The equilibrium constant of the reaction is $\frac{x}{15}$. The value of x is:

1. 24

2. 13

3. 16

4. 19

Given that the equilibrium constant (K_C) at 800 K for the reaction \(N_2(𝑔)+3H_2(𝑔)⇋2NH_3(𝑔)\) is 64. What is the equilibrium constant K_C at the same temperature for the reaction \(NH_3(g) ⇌ \dfrac{1}{2}N_2(g) + \dfrac{3}{2}H_2(g)\)?

For the following reactions, equilibrium constants are given below:

S_(s) + O_2(g) $\rightleftharpoons$SO_2(g); K₁ = 10⁵²

2S_(s) + 3O_2(g) $\rightleftharpoons$2SO_3(g); K₂ = 10¹²⁹

The equilibrium constant for the reaction, 2SO_2(g) + O_2(g) $\rightleftharpoons$2SO_3(g) is:

The equilibrium constant at 298 K for a reaction A + B  ⇋ C + D is 100.
If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L^–1) will be :

A vessel at 1000 K contains CO₂ with a pressure of 0.5 atm. Some of the CO₂ is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of K is :

1. 1.8 atm

2. 3 atm

3. 0.3 atm

4. 0.18 atm

In a closed reaction vessel, Phosphorus pentachloride dissociates as follows:

\(\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)\)

If the total pressure at equilibrium of the reaction mixture is P and the degree of dissociation of PCl₅  is x, the partial pressure of PCl₃ will be:

1. \(\left(\frac{x}{x+1}\right) P\)

2. \(\left(\frac{2x}{x-1}\right) P\)

3. \(\left(\frac{x}{x-1}\right) P\)

4.  \(\left(\frac{x}{1-x}\right) P\)

Consider the reaction equilibrium :  \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) ; \quad \Delta H^{\circ}=-198 \mathrm{~kJ} \)

On the basis of Le-Chatelier's principle, the condition favorable for the forward reaction is : 

1. lowering of temperature as well as pressure 

2. increasing temperature as well as pressure 

3. lowering the temperature and increasing the pressure 

4. Any value of temperature and pressure 

For the gaseous equilibrium reaction:
\({N_2O_4 (g) \rightleftharpoons 2NO_2 (g)}\), the equilibrium concentrations of \(\mathrm{N_2O_4}\) and \(\mathrm{NO_2}\)​ are \(4.8 \times 10^{-2}\) and \(1.2 \times 10^{-2}\), respectively.

Calculate the value of the equilibrium constant \(K_c\)​ for the reaction:

1. 3.3 \(\times\) 10²  mol L^-1
2. 3 \(\times\) 10^-1  mol L^-1
3. 3 \(\times\) 10^-3  mol L^-1
4. 3 \(\times\) 10³ mol L^-1