Given a system: $A\left(\mathrm{s}\right)\stackrel{ }{\rightleftharpoons }2B\left(\mathrm{g}\right) + 3C\left(\mathrm{g}\right).$ 
If the concentration of C at eqilibrium is increased by a factor 2, it will cause the eqilibrium concentration of B to change to:

1. two times of its original value

2. one half of its original value

3. 2$\sqrt{2}$ times of its original value

4. $\frac{1}{2\sqrt{2}}$ times of its original value

For the equilibrium, PCl₅ $\rightleftharpoons$ PCl₃ + Cl₂,

${\mathrm{K}}_{\mathrm{C}}={\mathrm{\alpha }}^2/(1-\mathrm{\alpha })\mathrm{V}$, temperature remaining constant:

1. K_c will increase with the increase in volume

2. K_c will increase with the decrease in volume

3. K_c will not change with the change in volume

4. K_c may increase or decrease with the  change in volume depending upon its numerical value.

In the dissociation of 2HI $\rightleftharpoons$H₂ + I₂, the degree of dissociation will be influenced by the:

1. Addition of inert gas at constant volume

2. Addition of inert gas at constant pressure

3. Increase of temperature

4. Increase of pressure

The correct order of increasing [H₃O⁺] in the following aqueous solutions is:

1. 0.01 M H₂S < 0.01 M H₂SO₄<0.01 M NaCl<0.01M NaNO₂

2. 0.01 M NaCl< 0.01 M NaNO₂<0.01 M H₂S< 0.01 M H₂SO₄

3. 0.01 M NaNO₂<0.01 M NaCl<0.01 M H₂S<0.01 M H₂SO₄

4. 0.01 M H₂S<0.01 M NaNO₂<0.01 M NaCl<0.01 M H₂SO₄

The pK_a of acetylsalicylic acid (aspirin) is 3.5. The pH of gastric juice in the human stomach is about 2-3 and the pH in the small intestine is about 8. Aspirin will be:

1. Unionized in the small intestine and in the stomach

2. Completely ionized in the small intestine and in the stomach

3. Ionized in the stomach and almost unionized in the small intestine

4. Ionized in the small intestine and almost unionized in the stomach