Find the acid dissociation constant (Kₐ) of HXO given that:

XO⁻(aq) + H₂O(l) ⇌ HXO(aq) + OH⁻(aq)

K = 0.36 × 10⁻⁶

1. 0.36 × 10⁻⁸
2.  2.8 × 10⁻⁸
3.  2.8 × 10⁻¹⁰
4. 0.36 × 10⁻⁶

 

The equilibrium constant value for the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>1.48\times {10}^{-5}$, the value for the reaction $1/2{\mathrm{N}}_2\left(\mathrm{g}\right)+3/2{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>\mathrm{n}\times {10}^{-3}$ where n is

1. 1.85

2. 3.85

3. 4.85

4. 10

A gaseous phase reaction is allowed to attain equilibrium as $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right)$ at constant pressure P. The partial pressure of A at equilibrium is P/2. The value of equilibrium constant K_p is

1. $\frac{\mathrm{P}}{8}$

2. $\frac{\mathrm{P}}{6}$

3. $\frac{\mathrm{P}}{2}$

4. $\frac{\mathrm{P}}{4}$

Two moles of N₂O₄ is heated to form NO and O₂. As soon as NO and O₂ are formed they react to form N₂O₅. Two equilibria

${\mathrm{N}}_2{\mathrm{O}}_4\rightleftharpoons 2\mathrm{NO}+{\mathrm{O}}_2$
$2\mathrm{NO}+\frac{3}{2}{\mathrm{O}}_2\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_5$

Are simultaneously established. At equilibrium, the degree of dissociation of N₂O₄ was found to 50%. Which of the following is correct at equilibrium?

1. $\frac{1}{2}\left[\mathrm{NO}\right]=\frac{3}{2}\left[{\mathrm{O}}_2\right]$

2. $2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]=\left[\mathrm{NO}\right]+\frac{3}{2}\left[{\mathrm{O}}_2\right]+\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]$

3. $\left[\mathrm{NO}\right]+\left[{\mathrm{O}}_2\right]=\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]+\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]$

4. $\frac{1}{2}\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]+\left[{\mathrm{O}}_2\right]=\frac{1}{2}\left[\mathrm{NO}\right]$

Find Kₚ for the following equilibrium at 25°C:

NH₄HS(s) ⇌ NH₃(g) + H₂S(g)

The total equilibrium pressure is 0.660 atm.

1. 0.109

2. 0.218

3. 1.89

4. 2.18

PCl₅ is 50% dissociated at $20°\mathrm{C}$ and 1 atm pressure. The value of K_p for this reaction is:

Find the equilibrium concentrations of SO₂ and SO₃ for the reaction:

SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

Given Kc = 16. Initially, 1 mol each of SO₂, NO₂, SO₃ and NO is taken in a 1 L vessel.

1. 0.4, 0.8

2. 0.8, 0.16

3. 1.6, 0.8

4. 0.4, 1.6

The ratio of \({{K_{P}}\over{K_{C}}}\) for the reaction

$\mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)$ $\mathrm{is:}$

Determine the value of equilibrium constant (K_c) for the reaction

${\mathrm{A}}_2\left(\mathrm{g}\right)+{\mathrm{B}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{AB}\left(\mathrm{g}\right)$

If 10 moles of A₂; 15 moles of B₂ and 5 moles of AB are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of AB is 7.5 M:

1. 4.5

2. 1.5

3. 0.6

4. None of the above

A 1 M solution of glucose reaches dissociation equilibrium given below.

${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\rightleftharpoons 6\mathrm{HCHO}$

If the equilibrium constant is $0.167x{10}^{-22}$, the concentration of HCHO in the equilibrium is

1. $1.60\times {10}^{-8<mspace\; width="1em"></mspace>}\mathrm{M}$

2. $3.20\times {10}^{-6}<mspace\; width="1em"></mspace>\mathrm{M}$

3. $3.20\times {10}^{-4}<mspace\; width="1em"></mspace>\mathrm{M}$

4. $1.60\times {10}^{-4}<mspace\; width="1em"></mspace>\mathrm{M}$