The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 90.0 °C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H2O, = 6.01 kJ/mol, and = 40.67 kJ/mol.

Question

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 90.0 °C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H2O,    = 6.01 kJ/mol, and  = 40.67 kJ/mol.

jfraser · Answer

You have to break this up into three parts.

How much heat is needed to bring the water from -25C to 0C, at which point it will begin to melt?

How much heat is needed to actually melt the ice?

How much heat is needed to bring the water from 0C to 90C?