Enthalpy of Phase Transition — MCQ Practice

Calculate the total heat required to convert $10,\text{g}$ of ice at $-10^circ\text{C}$ to steam at $120^circ\text{C}$. Given: Specific heat of ice ($c_{ice}$) = $2.1,\text{J/g}^circ\text{C}$ Specific heat of water ($c_{water}$) = $4.2,\text{J/g}^circ\text{C}$ Specific heat of steam ($c_{steam}$) = $2.0,\text{J/g}^circ\text{C}$ Enthalpy of fusion of ice ($Delta H_{fus}$) = $334,\text{J/g}$ Enthalpy of vaporization of water ($Delta H_{vap}$) = $2260,\text{J/g}$

Which of the following relationships is correct for the enthalpy changes of phase transitions?

Which of the following processes is exothermic?

Which factor primarily determines the magnitude of the enthalpy of vaporization of a substance?

When $1,\text{mol}$ of a liquid freezes at its freezing point, what can be said about the enthalpy change?

Given the following standard enthalpy changes: $ext{H}_2\text{O(s)} \rightarrow \text{H}_2\text{O(l)} quad Delta H_1 = +6.01,\text{kJ/mol}$ $ext{H}_2\text{O(l)} \rightarrow \text{H}_2\text{O(g)} quad Delta H_2 = +40.7,\text{kJ/mol}$ Calculate the standard enthalpy of deposition of water ($ext{H}_2\text{O(g)} \rightarrow \text{H}_2\text{O(s)}$).