Chemistry

Chemistry

Problem

For water, ΔHfus=6.01 kJ mol−1\Delta H_{\mathrm{fus}} = 6.01\,\text{kJ\,mol}^{-1} at 0 ∘C0\,^\circ\text{C} and ΔHvap=40.7 kJ mol−1\Delta H_{\mathrm{vap}} = 40.7\,\text{kJ\,mol}^{-1} at 100 ∘C100\,^\circ\text{C}. Assuming the enthalpies are temperature-independent, what is the molar enthalpy change for sublimation of ice at 0 ∘C0\,^\circ\text{C}, and how would this appear on an energy diagram? a) 40.7 kJ mol−140.7\,\text{kJ\,mol}^{-1} absorbed; single upward arrow from solid to gas. b) 46.7 kJ mol−146.7\,\text{kJ\,mol}^{-1} released; single downward arrow from gas to solid. c) 46.7 kJ mol−146.7\,\text{kJ\,mol}^{-1} absorbed; single upward arrow from solid to gas. d) 34.7 kJ mol−134.7\,\text{kJ\,mol}^{-1} absorbed; single upward arrow from solid to gas.

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