Question

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

Substance	Specific heat [J/(g⋅∘C)][J/(g⋅∘C)]	ΔHΔH (kJ/mol)(kJ/mol)
water	4.18	44.0
ice	2.01	6.01

a) Calculate the enthalpy change, ΔHΔHDeltaH, for the process in which 42.3 gg of water is converted from liquid at 3.2 ∘C∘C to vapor at 25.0 ∘C∘C . For water, ΔHvapΔHvapH = 44.0 kJ/molkJ/mol at 25.0 ∘C∘C and CsCsC_s = 4.18  J/(g⋅∘C) J/(g⋅∘C) for H2O(l)H2O(l).

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

b) How many grams of ice at -26.3 ∘C∘C can be completely converted to liquid at 9.0 ∘C∘C if the available heat for this process is 5.41×10³ kJkJ ?

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

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