4 public questions tagged with this topic.
For an isothermal process (Δ U = 0), Δ U = q + w = 0, so q = -w. For reversible compression, w = -nRT ln(V₂/V₁) (positive), so q = nRT ln(V₂/V₁), which is negative since V₂ < V₁.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Gibbs Energy and Gibbs Energy Change and Equilibrium
For isothermal process, Δ U = 0, so q = -w. Compression means w > 0 (4988 J), so q = -4988 J.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Enthalpy Changes - Reaction Formation Combustion and Hess's Law
Δ S = nR ln(V₂/V₁) = 1 × 8.314 × ln(5/20) = 8.314 × ln(0.25) = 8.314 × (-1.386) = -11.52 J/K.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Bond Enthalpy and Entropy and Spontaneity
Δ S = nR ln(V₂/V₁) = 1 × 8.314 × ln(5/10) = 8.314 × (-0.693) = -5.76 J/K.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Bond Enthalpy and Entropy and Spontaneity
