q1 = heat to move ice from -12 C to zero C.
q1 = mass ice x specific heat ice x (Tfinal-Tinitial). Note Tfinal = 0 and Ti = -12 so 0-(-12) = +12.
q2 = heat needed to melt ice at zero C to liquid water at zero C.
q2 = mass ice x heat fusion.
q3 = heat to move T of liquid water from zero C to 32 C,.
q3 = mass x specific heat water x (Tfinal-Tinitial).
Total q = q1 + q2 + q3.
How much energy (in kilojoules) is needed to heat 5.45g of ice from -12.0 C to 32.0 C? The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K x mol) for ice and 75.3 J/(k x mol) for liquid water
2 answers
15kj