Which of the following gaseous equilibria has Kp less than Kc?

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

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

3. $2\mathrm{HI}\rightleftharpoons {\mathrm{H}}_2+{\mathrm{I}}_2$

4. ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons {\mathrm{NH}}_3$

The value of K_c for the reaction  \(\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})\) at 400 is 0.5.
The value of K_p for the reactions is: $(\mathrm{R}=0.0821<mspace\; width="1em"></mspace>\mathrm{L}<mspace\; width="1em"></mspace>\mathrm{atm}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1})$

1. $25.6\times {10}^{-2}$

2. $4.6\times {10}^{-4}$

3. $46.6\times {10}^{-4}$

4. $16.6\times {10}^{-8}$

The value of K_p for the reaction,

$2{\mathrm{SO}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)\hspace{0.17em}+{\mathrm{O}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{SO}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>700<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>1.3\times {10}^{-3}<mspace\; width="1em"></mspace>{\mathrm{atm}}^{-1}.$ The value of K_c at same temperature will be

1. $1.4\times {10}^{-2}$

2. $7.4\times {10}^{-2}$

3. $5.2\times {10}^{-2}$

4. $3.1\times {10}^{-2}$

The ratio of $\frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}$for the reaction

${\mathrm{SO}}_2\left(\mathrm{g}\right)+{\displaystyle \frac{1}{2}}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}$

1. (RT)^-1/2 

2. (RT)^1/2 

3. (RT)

4. 1

$\mathrm{If}<mspace\; width="1em"></mspace>2\underset{\mathrm{g}}{\mathrm{NO}}\rightleftharpoons {\mathrm{N}}_2+{\mathrm{O}}_2$
${\mathrm{K}}_{{\mathrm{c}}_1}=2.5\times {10}^{30}$
$\underset{\mathrm{g}}{\mathrm{NO}}+\frac{1}{2}\underset{\mathrm{g}}{{\mathrm{Br}}_2}\rightleftharpoons \underset{\mathrm{g}}{\mathrm{NOBr}}$
${\mathrm{K}}_{{\mathrm{c}}_2}=1.6$

find K_c for the reaction given below

$\frac{1}{2}\underset{\mathrm{g}}{{\mathrm{N}}_2}+\frac{1}{2}\underset{\mathrm{g}}{{\mathrm{O}}_2}+\frac{1}{2}\underset{\mathrm{g}}{{\mathrm{Br}}_2}\rightleftharpoons \underset{\mathrm{g}}{\mathrm{NOBr}}$

1. $1.01\times {10}^{-15}$

2. $2.02\times {10}^{-15}$

3. $1.01\times {10}^{30}$

4. $2.02\times {10}^{15}$

If K_p of the reaction $\mathrm{A}\left(\mathrm{g}\right)+2\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 3\mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$ is 0.05 at 1000 K, then the value of K_c of the reaction

1. 20000 R

2. 0.02 R

3. $\frac{5\times {10}^{-5}}{\mathrm{R}}$

4. $5\times {10}^{-5}\mathrm{R}$

What will be the change in the concentration of Cl₂ when the equilibrium concentration of PCl₃ is doubled in the reaction:

PCl₅(s) ⇌ PCl₃(g) + Cl₂(g)?

1. Cl₂ becomes half of its initial concentration

2. Cl₂ becomes one-fourth of its initial concentration

3. Cl₂ becomes four times its initial concentration

4. Cl₂ becomes twice its initial concentration

In the reaction, the equilibrium concentrations of PCl₅ and PCl₃ are 0.4 and 0.2 mole/liter respectively. If the value of K_c is 0.5, what is the concentration of Cl₂ in mole/liter?

1. 2.0

2. 1.5

3. 1.0

4. 0.5

4 moles each of SO₂ and O₂ gases are allowed to react to form SO₃ in a closed vessel. At equilibrium, 25% of O₂ is used up. The total number of moles of all the gases at equilibrium is

1. 6.5

2. 7.0

3. 8.0

4. 2.0

For the reversible reaction,

N2(g)+3H2(g)⇌2NH3(g)

At 500°C, the value of K_p is 1.44×10^-5 when partial pressure is measured in atmospheres. The corresponding value of K_c, with concentration in mole L^-1, is

1. 1.44×10^-5(0.082×500)^-2

2. 1.44×10^-5/(8.314×773)^-2

3. 1.44×10^-5(0.082×773)^-2

4. 1.44×10^-5/(0.082×773)^-2