Draw a heating curve (such as the one in Figure 11.36) for 1 mol ...

Question

Draw a heating curve (such as the one in Figure 11.36) for 1 mol of benzene beginning at 0 °C and ending at 100 °C. Assume that the values given here are constant over the relevant temperature ranges: Melting point 5.4 °C, Boiling point 80.1 °C, ΔHfus 9.9 kJ/mol, ΔHvap 30.7 kJ/mol, Cs,solid 118 J/mol⋅K, Cs,liquid 135 J/mol⋅K, Cs,gas 104 J/mol⋅K.

Accepted Answer

Identify the key points on the heating curve: the melting point at 5.4 °C and the boiling point at 80.1 °C.. Calculate the energy required to heat the solid benzene from 0 °C to its melting point using the formula: $ q = m \cdot C_{s,solid} \cdot \Delta T $, where $ m $ is the number of moles, $ C_{s,solid} $ is the specific heat capacity of solid benzene, and $ \Delta T $ is the temperature change.. Calculate the energy required for the phase change from solid to liquid at the melting point using the formula: $ q = m \cdot \Delta H_{fus} $, where $ \Delta H_{fus} $ is the enthalpy of fusion.. Calculate the energy required to heat the liquid benzene from its melting point to its boiling point using the formula: $ q = m \cdot C_{s,liquid} \cdot \Delta T $.. Calculate the energy required for the phase change from liquid to gas at the boiling point using the formula: $ q = m \cdot \Delta H_{vap} $, where $ \Delta H_{vap} $ is the enthalpy of vaporization.