Which of the following conditions leads to Kp being less than Kc?

1. ${\mathrm{N}}_2+{\mathrm{O}}_2\rightleftharpoons 2\mathrm{NO}$

2. ${\mathrm{H}}_2+{\mathrm{Cl}}_2\rightleftharpoons 2\mathrm{HCl}$

3. $2{\mathrm{SO}}_2+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3$

4. ${\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3+{\mathrm{Cl}}_2$

Equilibrium constants K₁, and K₂ for the following equilibria

$\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\stackrel{{\mathrm{K}}_1}{\rightleftharpoons }{\mathrm{NO}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{and}$
$2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2$

are related as

1. ${\mathrm{K}}_2=1/{\mathrm{K}}_1^2$

2. ${\mathrm{K}}_2={\mathrm{K}}_1^2$

3. ${\mathrm{K}}_2=1/{\mathrm{K}}_1$

4. ${\mathrm{K}}_2={\mathrm{K}}_1/2$

In a chemical equilibrium rate constant of forward reaction is $7.5\times {10}^{-4}$ and the equilibrium constant is 1.5. The rate constant of a backward reaction is

1. $2.5\times {10}^4$

2. $5\times {10}^{-4}$

3. $2.5\times {10}^{-4}$

4. $5\times {10}^4$

$\underset{\mathrm{g}}{{\mathrm{PCl}}_5}\rightleftharpoons \underset{\mathrm{g}}{{\mathrm{PCl}}_3}+\underset{\mathrm{g}}{{\mathrm{Cl}}_2}$

For the dissociation of PCl_5- K_c is $2\times {10}^{-7}<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>27°\mathrm{C}$.

$\mathrm{Find}<mspace\; width="1em"></mspace>∆\mathrm{S}°<mspace\; width="1em"></mspace>\mathrm{If}<mspace\; width="1em"></mspace>∆\mathrm{H}°=28.4<mspace\; width="1em"></mspace>\mathrm{KJ}/\mathrm{m}$

1. -0.0336 KJ/K

2. 0.0336 KJ/K

3. -0.0818 KJ/K

4. 0.338 KJ/K

The value of K_p for the reaction,

$2{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{S}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>1.2\times {10}^{-2}<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>1065°\mathrm{C}.$

The value of K_c is

1. $<1.2\times {10}^{-2}$

2. $>1.2\times {10}^{-2}$

3. $1.2\times {10}^{-2}$

4. $0.12\times {10}^{-2}$

What volumes of H₂ and NH₃ are required or formed when 100 mL of N₂ reacts completely in the reaction
N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?

1. 300 mL of H₂ and 300 mL of NH₃ 

2. 100 mL of H₂ and 200 mL of NH₃ 

3. 300 mL of H₂ and 200 mL of NH₃ 

4. 100 mL of H₂ and 100 mL of NH₃ 

Find the ratio of volumes of reactants and products when a mixture containing 3 moles of hydrogen and 1 mole of nitrogen is completely converted into ammonia at the same temperature and pressure.

1. 2:1

2. 1:2

3. 1:3

4. 3:1

Find the equilibrium constant for the reaction 2A(g) ⇌ B(g) + C(g) at 780 K, given that Kp = 3.52 at 10 atm.
What is the value of Kp when the pressure is increased to 20 atm at the same temperature?

1. 5.72

2. 11.44

3. 28.6

4. 3.52

For the reaction, $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$, the rate constants for the forward and backward reactions are found to be $4.2\times {10}^{-2}$ and $3.36\times {10}^{-3}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{s}}^{-1}$ respectively. What is the equilibrium constant for the reaction?

1. 11.5

2. 12.5

3. 8.0

4. 6.0

In the reaction $2{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{S}}_2\left(\mathrm{g}\right)$ the concentration of H₂S is 0.5 mol L^-1 and concentration of H₂ is 0.1 mol L^-1 while concentration of S₂ is 0.4 mol L^-1 in one litre vessel. The value of equilibrium constant of the reaction is

1. 0.016

2. 0.013

3. 0.020

4. 0.030