# Problem: How many grams of ice at -9.1 ∘C can be completely converted to liquid at 16.4°C if the available heat for this process is 5.69×103 kJ?For ice, use a specific heat of 2.01 J/ (g°C) and ΔHfus = 6.01 kJ/ mol .Express your answer to three significant figures and include the appropriate units.Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change q = m Cs ΔTwhere Cs is specific heat and mm is mass.Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase changeq = n ⋅ ΔHwhere, nn is the number of moles and ΔH is the enthalpy of fusion, vaporization, or sublimation.The following table provides the specific heat and enthalpy changes for water and ice.

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How many grams of ice at -9.1 ∘C can be completely converted to liquid at 16.4°C if the available heat for this process is 5.69×103 kJ?

For ice, use a specific heat of 2.01 J/ (g°C) and ΔHfus = 6.01 kJ/ mol .

Express your answer to three significant figures and include the appropriate units.

Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change

q = m Cs ΔT
where Cs is specific heat and mm is mass.

Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change

q = n ⋅ ΔH

where, nn is the number of moles and ΔH is the enthalpy of fusion, vaporization, or sublimation.

The following table provides the specific heat and enthalpy changes for water and ice. 