Exams › JEE Advanced › Chemistry

For the equilibrium PCl5(g) <=> PCl3(g) + Cl2(g), an increase in pressure causes:

1. An increase in degree of dissociation and a decrease in Kc
2. A decrease in degree of dissociation and a decrease in Kc
3. An increase in degree of dissociation but Kc remains constant
4. A decrease in degree of dissociation but Kc remains constant

Correct answer: A decrease in degree of dissociation but Kc remains constant

Solution

Higher pressure shifts the equilibrium toward the reactant side (fewer moles), decreasing the degree of dissociation, while Kc is unchanged because it depends only on temperature.

Related JEE Advanced Chemistry questions

• In which of the following cases can the pH be determined using the equilibrium constant(s) provided?
• In the equilibrium reaction NH2COONH4(s) ⇌ 2NH3(g) + CO2(g), which change will cause the partial pressure of NH3 to rise?
• For the reaction XY2(g) ⇌ XY(g) + Y(g), if the value of α (degree of dissociation) is very small compared to 1, how is α related to the pressure (P)?
• At 460°C, 0.02 g of hydrogen reacts with 2.54 g of iodine until equilibrium is reached. Upon analysis, the equilibrium mixture contains 0.0021 moles of iodine. What is the equilibrium constant (Kc) for this reaction?
• Determine the pH of a 1.0 M solution of an unidentified hydroxide compound, assuming the metal ion has a +1 charge.
• What explains the acidic nature of an aqueous solution of aluminum chloride?

⚔️ Practice JEE Advanced Chemistry free + battle 1v1 →