Calculate the heat absorbed when 46.0 g of ice at -10.0°C is converted to liquid water at 85.0 °C. The specific heat of ice is 2.03 J/g °C, the molar heat of fusion of ice is 6010 J/mol, and the specific heat of water is 4.18 °J/g °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:

Calculate the heat released when 65.5 g of steam at 116.0°C is converted to water at 57.0°C. Assume that the specific heat of water is 4.184 J/g ·°C, the specific heat of steam is 1.99 J/g ·°C,and ΔHvap = 40.79 kJ/mol for water.

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

How much heat (in joules) must be added to change 20.0 g of H2O(s) at –10.0°C to steam at 110.0°C? The specific heat of H2O(s) is 2.09 J/g °C, of H2O(l) is 4.184 J/g °C, and of H2O(g) is 1.84 J/g °C. The heat of fusion of water is 334.7 J/g and the heat of vaporization is 2259.4 J/g

Two 20.0 g ice cubes at -18.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Tf = °C

Calculate the heat released when 25.0 g of steam becomes liquid water at 100.0°C. The molar heat of vaporization of water is 4.07 x 10 4 J/mol.

Specific heat of H,O(s) 2.087 J/(g · °C) Specific heat of H,O(1) |4.184 J/ (g · °C) Heat of fusion for H,O A total of 865 cal of heat is added to 5.00 g of ice at -20.0 °C. 333.6 J/g What is the final temperature of the water? °C Tinal

How much heat (in kJ) is released in converting 1.00 mol of water as a gas at 105°C to ice at –5.0°C? The heat capacity of H2O (g) is 2.01 J/g · °C The heat capacity of H2O (l) is 4.18 J/g · °C The heat capacity of H2O (s) is 2.09 J/g · °C The heat of fusion for water at 0 °C is approximately 0.334 kJ/g The heat of vaporization for water at 100 °C is 2.230 kJ/g.

How much heat must be supplied to 36 g of ice at -21°C to convert it to steam at 152°C? (Specific heats: ice = 2.0 J/g·°C; water = 4.2 J/g·°C; steam = 2.0 J/g·°C. Molar heat of fusion of water at 273 K = 6.01 kJ/mol. Molar heat of vaporization of water at 373 K = 40.7 kJ/mol.)