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

Question

Draw a heating curve (such as the one in Figure 11.36) for 1 mole of methanol beginning at 170 K and ending at 350 K. Assume that the values given here are constant over the relevant temperature ranges. Melting point: 176 K, Boiling point: 338 K, ΔH_fus: 2.2 kJ/mol, ΔH_vap: 35.2 kJ/mol, C_s,solid: 105 J/mol·K, C_s,liquid: 81.3 J/mol·K, C_s,gas: 48 J/mol·K.

Accepted Answer

Identify the different phases and phase transitions of methanol between 170 K and 350 K: solid, liquid, and gas phases, with melting at 176 K and boiling at 338 K.. Calculate the energy required to heat the solid methanol from 170 K to its melting point at 176 K 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 methanol, and $ \Delta T $ is the temperature change.. Determine the energy needed for the phase transition 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 methanol from 176 K to its boiling point at 338 K using the formula: $ q = m \cdot C_s,liquid \cdot \Delta T $, where $ C_s,liquid $ is the specific heat capacity of liquid methanol.. Determine the energy needed for the phase transition 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.