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.

anonymous · Answer

because ice absorb calor so enthalpy will go up..
$$\Delta H = Q$$
$$Q= (mc \Delta t )ice+ mL + (mc \Delta t) water$$
L=334 J/g , m ice = m water