NEET Equilibrium — Set 6

Question 1

For $ \ce{SO2(g) + Cl2(g) <=> SO2Cl2(g)} $, $ K_c = 16 $ at 400 K. If 0.3 mol $ \ce{SO2} $ and 0.2 mol $ \ce{Cl2} $ are in a 1 L vessel, what is $ [\ce{SO2Cl2}] $ at equilibrium?

Accepted Answer

Initial: $ [\ce{SO2}] = 0.3 \, \text{M} $, $ [\ce{Cl2}] = 0.2 \, \text{M} $, $ [\ce{SO2Cl2}] = 0 $. Let $ x = [\ce{SO2Cl2}] $, $ [\ce{SO2}] = 0.3 - x $, $ [\ce{Cl2}] = 0.2 - x $. $ K_c = \frac{[\ce{SO2Cl2}]}{[\ce{SO2}][\ce{Cl2}]} = \frac{x}{(0.3 - x)(0.2 - x)} = 16 $, $ x = 16 (0.06 - 0.5x + x^2) $, $ x \approx 0.18 \, \text{M} $.

Question 2

A solution has $ [\ce{H+}] = 2.0 \times 10^{-4} \, \text{M} $. What is its pH?

Accepted Answer

$ \text{pH} = -\log[\ce{H+}] = -\log(2.0 \times 10^{-4}) = 4 - \log 2 \approx 4 - 0.3010 = 3.7 $.

Question 3

Which law relates the partial pressure of a gas to its solubility in a liquid?

Accepted Answer

Henry’s Law states that the solubility of a gas in a liquid is directly proportional to its partial pressure above the liquid.

NEET Chemistry: Equilibrium — Practice Set 6

Q1. For \( \ce{SO2(g) + Cl2(g) <=> SO2Cl2(g)} \), \( K_c = 16 \) at 400 K. If 0.3 mol \( \ce{SO2} \) and 0.2 mol \( \ce{Cl2} \) are in a 1 L vessel, what is \( [\ce{SO2Cl2}] \) at equilibrium?

Q2. A solution has \( [\ce{H+}] = 2.0 \times 10^{-4} \, \text{M} \). What is its pH?

Q3. Which law relates the partial pressure of a gas to its solubility in a liquid?

Q4. For \( \ce{2HI(g) <=> H2(g) + I2(g)} \), \( K_p = 0.04 \) at 500 K. If 1 mole of \( \ce{HI} \) is placed in a 1 L vessel, what is the total pressure at equilibrium (\( R = 0.0831 \, \text{bar L/mol K} \))?

Q5. For \( \ce{2NO(g) + O2(g) <=> 2NO2(g)} \), \( K_c = 100 \) at 300 K. If 0.2 mol \( \ce{NO} \) and 0.1 mol \( \ce{O2} \) are in a 1 L vessel, what is \( [\ce{NO2}] \) at equilibrium?

Q6. For \( \ce{2X(g) <=> Y(g) + Z(g)} \), \( K_c = 0.01 \) at 400 K. If 1 mol \( \ce{X} \) is in a 1 L vessel, what is the degree of dissociation at equilibrium?

Q7. Which species can act as both a Lewis acid and base?

Q8. For \( \ce{AgCl(s) <=> Ag+(aq) + Cl-(aq)} \), \( K_{sp} = 1.8 \times 10^{-10} \). In a 0.05 M \( \ce{KCl} \) solution, what is \( [\ce{Ag+}] \) at equilibrium?

Q9. The \( \text{p}K_a \) of a weak acid is 5.2. What is its \( K_a \)?

Q10. A weak base \( \ce{BOH} \) (\( K_b = 5.0 \times 10^{-6} \)) has a 0.02 M solution with 0.5% ionization. What is the pH?