4 public questions tagged with this topic.
Halving volume doubles concentrations: Q = ((1.8)³/(0.6)² (0.2)) = 81 > 9 , shifts left.
Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Physical Equilibrium - Solid-Liquid Gas-Liquid and Henry's Law
Increasing pressure (decreasing volume) favors the side with fewer moles of gas. Here, 2 mol → 2 mol , so Δ n = 0 , and there is no shift.
Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant
Increasing pressure (halving volume) favors the side with fewer moles of gas. Here, 2 mol → 2 mol , Δ n = 0 , so there is no shift.
Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Chemical Equilibrium - Law of Mass Action and Equilibrium Constant
T₂ = T₁ (V₁/V₂)γ⁻¹ = 500 × (8/16)⁰.³³ = 500 × (0.5)⁰.³³ = 500 × 0.793 = 396.5 K.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Gibbs Energy and Gibbs Energy Change and Equilibrium
