Question

Calculating entropy change from reversible heat flow The heat of fusion ?Hf of acetone (OC(CH3)2) is 5.7 kJ/mol. Calculate the change in entropy ?S when 2.8 g of acetone melts at -94.7 °C. Be sure your answer contains a unit symbol and the correct number of significant digits.

          Calculating entropy change from reversible heat flow
The heat of fusion ?Hf of acetone (OC(CH3)2) is 5.7 kJ/mol. Calculate the change in entropy ?S when 2.8 g of acetone melts at -94.7 °C. Be sure your answer contains a unit symbol and the correct number of significant digits.

Calculating entropy change from reversible heat flow
The heat of fusion ?Hf of acetone (OC(CH3)2) is 5.7 kJ/mol. Calculate the change in entropy ?S when 2.8 g of acetone melts at -94.7 °C. Be sure your answer contains a unit symbol and the correct number of significant digits.

Added by Victoria C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

07/15/2022

Step 1

Given: Heat of fusion of acetone (ΔHf) = 5.7 kJ/mol Temperature (T) = 94.7°C = 94.7 + 273.15 = 367.85 K Using the equation ΔG = ΔH - TΔS and knowing that ΔG = 0 at equilibrium: 0 = 5.7 - 367.85ΔS ΔS = 5.7 / 367.85 ΔS = 0.0155 kJ/mol K = 15.5 J/mol K ** Show more…

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Calculating entropy change from reversible heat flow The heat of fusion ΔHf of acetone (OC(CH3)2) is 5.7 kJ/mol. Calculate the change in entropy ΔS when 2.8 g of acetone melts at -94.7 °C. Be sure your answer contains a unit symbol and the correct number of significant digits.