The heat of fusion \( \Delta H_{f} \) of benzene \( \left(\mathrm{C}_{6} \mathrm{H}_{6}\right) \) is \( 10.6 \mathrm{~kJ} / \mathrm{mol} \). Calculate the change in entropy \( \Delta S \) when \( 869 . \mathrm{g} \) of benzene melts at \( 5.6{ }^{\circ} \mathrm{C} \). Be sure your answer contains a unit symbol. Round your answer to 3 significant digits.
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\[ \text{Molar mass of C} = 12.01 \, \text{g/mol} \] \[ \text{Molar mass of H} = 1.01 \, \text{g/mol} \] \[ \text{Molar mass of C₆H₆} = 6 \times 12.01 + 6 \times 1.01 = 72.06 + 6.06 = 78.12 \, \text{g/mol} \] Show more…
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