4 KJ of heat is absorbed when 1 mol of ice melts at 0ºC and at constant pressure 1 atm. If molar volume of ice and water are 19 ml and 18 ml respectively, then [Take 1 atm = 105 Pa]

Engineering

Chemistry

Enthalpy and Internal Energy Relation

First Law and Various Process

Question

4 KJ of heat is absorbed when 1 mol of ice melts at 0ºC and at constant pressure 1 atm. If molar volume of ice and water are 19 ml and 18 ml respectively, then [Take 1 atm = 10⁵ Pa]

ΔU > ΔH

ΔU = 4.1 KJ

ΔU = 4.0001 KJ

ΔH > ΔU

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ΔH = 4 KJ

ΔH = ΔU + Δ(PV)

ΔU = 4 – P(V₂ – V₁)

$= 4 - \frac{10^{5} (18 - 19) \times 10^{- 6}}{10^{3}} = 4 + 1 \times 10^{- 4} = 4.0001 KJ$