How much heat is released ( in J) when 54.0 g of water at 10.0 °C is cooled to form ice at - 10.0 °C?  Molar mass of H2O = 18.0 g/mol Specific heat capacity of H2O(s) = 2.09 J/g. °C Specific heat capacity of H2O(l) = 4.18 J/g. °C ∆Hfus= 6.02 kJ/mol Boiling point of water is 100.0°C Freezing point of water is 0.0 °C

What amount of thermal energy (in kJ) is required to convert 221 g of ice at -16 °C completely to water vapour at 214 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-¹ The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-¹ The specific heat capacity of ice is 2.09 J g-¹ °C-¹ The specific heat capacity of liquid water is 4.18 J g-¹ °C-¹ The specific heat capacity of water vapour is 2.01 Jg¹¹ °C-¹ Answer:

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05  kg of water decreased from 117  °C to 56.5  °C.  Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C

How much energy would need to be added to 930.g of ice at 0.0°C to turn it into liquid water at 0.0°C ? 930. J O 3.89x103 J O 1.86x103 J O 2.10x106 J 3.12x105 J