Exams › JEE Advanced › Chemistry

For the industrial synthesis of nitric oxide via N2(g) + O2(g) ⇌ 2NO(g) (endothermic, ΔH > 0), the forward formation of NO is favoured by:

1. Increasing the pressure
2. Decreasing the pressure
3. Increasing the temperature
4. Decreasing the temperature

Correct answer: Increasing the temperature

Solution

Since moles of gas are equal on both sides, pressure changes do not shift the equilibrium. As the reaction is endothermic, raising the temperature shifts equilibrium toward NO.

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 →