A 25.5-g sample of ice at -10.0°C is mixed with 110.0 g water at 85.0°C. Calculate the final temperature (in °C) of the mixture assuming no heat loss to the surroundings. The heat capacities for H2O(I) and H2O(s) are 4.184 J/g °C and 2.03 J/g-°C, respectively, and the enthalpy of fusion of ice is 6.02 kJ/mol.

A 5.00 g sample of water vapor, initially at 155*C is cooled at atmospheric pressure, producing ice at -55*C. Calculate the amount of heat energy lost by the water vapor sample in this process, in kJ. Use the following data specific heat capacity of ice is 2.09 J/ gK; the specific heat capacity of liquid water is 4.18 J/ gK; the specific heat capacity of water vapor is 1.84 J/ gK; the heat of fusion of ice is 336 J/g; the heat of vaporization of water is 2260 J/g. ( I know the answer is 15.6 kJ but I don't know how to get to it, Pls help ASAP!!)show all the steps you can pls

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:

Two 20.0 g ice cubes at -14.0 °C are placed into 295 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

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

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.)