How much heat (in kJ) is evolved in converting 1.00 mol of steam at 145 °C to ice at -50 °C? The heat capacity of steam is 2.01 J/g°C, and that of ice is 2.09 J/g°C.

Verified step by step guidance

1. Calculate the heat lost by steam as it cools from 145 °C to 100 °C using q = m * C * ΔT, where m is the mass of steam, C is the heat capacity of steam, and ΔT is the change in temperature.
2. Determine the heat released during the phase change from steam to liquid water at 100 °C using q = n * ΔH_vap, where n is the number of moles and ΔH_vap is the enthalpy of vaporization.
3. Calculate the heat lost by water as it cools from 100 °C to 0 °C using q = m * C * ΔT, where C is the heat capacity of liquid water.
4. Determine the heat released during the phase change from liquid water to ice at 0 °C using q = n * ΔH_fus, where ΔH_fus is the enthalpy of fusion.
5. Calculate the heat lost by ice as it cools from 0 °C to -50 °C using q = m * C * ΔT, where C is the heat capacity of ice.