How much heat in Kj is released when 90.0 g of steam at 113 C is cooled to ice at -26 C?

Molar mass of H₂O = (1.0×2 + 16.0) g/mol = 18.0 g/mol
No. of moles of steam = (90.0 g) / (18.0 g/mol) = 5.00 mol

Energy released when 90.0 g steam at 113°C changes to steam at 100°C
= (90.0 g) × (1.84 J/g°C) × [(113 - 100)°C] × (1 kJ / 1000 J)
= 2.15 kJ

Energy released when steam condenses to water at 100°C
= (5.00 mol) × (40.67 kJ/mol)
= 203.35 kJ

Energy released when 90.0 g of water at 100°C to water at 0°C
= (90.0 g) × (4.184 J/g°C) × [(100 - 0)°C] × (1 kJ / 1000 J)
= 37.66 kJ

Energy released when 90.0 g of water changes to ice at 0°C
= (5.00 mol) × (6.01 kJ/mol)
= 30.05 kJ

Energy released when 90.0 g of ice at 0°C to ice at -26°C
= (90.0 g) × (2.903 J/g°C) × [0 - (-26)]°C × (1 kJ / 1000 J)
= 6.79 kJ

Total energy released
= (2.15 + 203.35 + 37.66 + 30.05 + 6.79) kJ
= 280 kJ