For a gaseous reaction ,$2\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D},$

the partial pressure of A, B, C and D at equilibrium are 0.5, 0.8, 0.7 and 1.2 atm. The value of K_p for this reaction is

1. 2.4 atm

2. 6.2 atm^-2

3. 4.2 atm^-1

4. 8.4 atm^-3

For the reaction $\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{CO}\left(\mathrm{g}\right),$ the partial pressure of CO₂ and CO are 4 and 8 atm respectively. The value of K_p for this reaction is

1. 14 atm

2. 16 atm

3. 18 atm

4. 12 atm

In which of the following gaseous reaction, K_p and K_c have the same values?

1. $2\mathrm{HI}\rightleftharpoons {\mathrm{H}}_2+{\mathrm{I}}_2$

2. ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$

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

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

Find the gaseous equilibrium for which Kp < Kc.

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. $16.6\times {10}^{-8}$

Find the value of Kc for the reaction:

2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

at 700 K, if

Kₚ = 1.3 × 10⁻³ atm⁻¹

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