Question:
Identify the reaction for which, at equilibrium, a change in the volume of the closed reaction vessel at a constant temperature will not affect the extent of the reaction
Identify the reaction for which, at equilibrium, a change in the volume of the closed reaction vessel at a constant temperature will not affect the extent of the reaction
Updated On: Jan 18, 2025
- CaCO3 (𝑠) ⇌ CaO(𝑠) + CO2(𝑔)
- H2 (𝑔) + I2 (𝑔) ⇌ 2HI(𝑔)
- 2NO2 (𝑔) ⇌ N2O4 (𝑔)
- CO2 (𝑠) ⇌ CO2 (𝑔)
Show Solution
Verified By Collegedunia
The Correct Option is B
Solution and Explanation
At equilibrium, the effect of a change in volume is determined by the number of gaseous moles on either side of the reaction.
- If the total number of gaseous moles changes during the reaction, a change in volume will shift the equilibrium to favor the side with more or fewer moles of gas (as per Le Chatelier’s principle).
- If the total number of gaseous moles remains the same, a change in volume will not affect the extent of the reaction.
Let’s analyze each option:
- (A) CaCO3(s) ⇌ CaO(s) + CO2(g) : This reaction involves a change in the number of moles of gas (0 → 1). Hence, a change in volume will affect the equilibrium.
- (B) H2(g) + I2(g) ⇌ 2HI(g) : The number of gaseous moles on both sides of the reaction is the same (2 → 2). Thus, a change in volume will not affect the equilibrium.
- (C) 2NO2(g) ⇌ N2O4(g) : This reaction involves a change in the number of gaseous moles (2 → 1). Hence, a change in volume will affect the equilibrium.
- (D) CO2(s) ⇌ CO2(g) : This reaction involves a change from a solid to a gas (0 → 1). Hence, a change in volume will affect the equilibrium.
Was this answer helpful?
1
0
Top IIT JAM CY Physical Chemistry Questions
- The diagram that best describes the variation of viscosity (𝜂) of water with temperature at 1 atm is
The SI unit of the molar conductivity of an electrolyte solution is
- The system with the lowest zero-point energy when it is confined to a one dimensional box of length 𝐿 is
- Adsorption of a gas on a solid surface follows the Langmuir isotherm. If \(\frac{ k_a}{k_d}\)=1.0 bar-1 , the fraction of adsorption sites occupied by the gas at equilibrium under 2.0 bar pressure of the gas at 25 °C is
( ka and kd are the rate constants for adsorption and desorption processes, respectively, at 25 °C) - The vapor pressure of a dilute solution of a non-volatile solute and the vapor pressure of the pure solvent at the same temperature are P and P*, respectively. \(\frac{P^*-P}{P^*}\) is equal to
(Assume that the vapor phase behaves as an ideal gas)
View More Questions
Top IIT JAM CY Thermodynamics Questions
- The correct relation(s) for an ideal gas in a closed system is/are
- Consider the following reaction:
2 C6H6+15 O2→12 CO2+6 H2O \(Δ_r𝐻^0_{298}\) =−3120 kJ mol−1.
A closed system initially contains 5 moles of benzene and 25 moles of oxygen under standard conditions at 298 K. The reaction was stopped when 17.5 moles of oxygen is left. The amount of heat evolved during the reaction is____kJ.
(round off to the nearest integer) - In the Born-Haber cycle, the heat of formation of CuCl is ______ kJ/mol.
[Given: Heat of atomization of Cu = +338 kJ/mol,
Ionization energy of Cu = +746 kJ/mol,
Heat of atomization of Cl2 = +121 kJ/mol,
Electron affinity of Cl = −349 kJ/mol, and
Lattice energy of CuCl = −973 kJ/mol]
(round off to the nearest integer) - The volume of 2.0 mol of an ideal gas is reduced to half isothermally at 300 K in a closed system. The value of ΔG is_____ kJ.
[Given: R=8.314 J mol-1 K-1 ]
(round off to two decimal places) - A system undergoes one clockwise cycle from point X back to point X as shown in the figure below:
The correct statement about this process is
View More Questions
Top IIT JAM CY Questions
- The structure of Q in the following reaction scheme is.
- The major product of the reaction is
- The rate of addition of 1-hexyl radical to the given molecules follows the order
- The major product of the reaction is
- The diagram that best describes the variation of viscosity (𝜂) of water with temperature at 1 atm is
View More Questions