How much heat is required to warm 1.50 L of water from 25.0 °C to 100.0 °C? (Assume a density of 1.0 g/mL for the water and a specific heat capacity of 4.18 J/g°C.)

Given that the heat of fusion of water is 6.02 kJ/mol, the heat capacity of H2O(l) is 75.2 J/mol·K, and the heat capacity of H2O(s) is 37.7 J/mol·K, calculate the total heat required to convert 1 mole of ice at -10°C to liquid water at 0°C.

How much energy is required to raise the temperature of 900 grams of water from 25°C to 100°C, given that the specific heat capacity of water is 4.18 J/g°C?

How much heat (in kJ) must be added to a sample of metal weighing 95.6 g for the temperature to change from 30.0 °C to 98.0 °C? The specific heat of the metal is 0.451 J/g°C.

How much heat in joules is required to raise the temperature of a 100.0 g piece of copper from 18°C to 35°C, given that the specific heat capacity of copper is 0.385 J/g°C?

How much heat is required to warm 2.80 kg of sand from 31.0 °C to 100.0 °C? The specific heat capacity of sand is 0.840 J/(g·°C). Express the heat in joules to three significant figures.

How much heat must be added to 25.0 g of water to raise the temperature from 15.0°C to 40.0°C? (Specific heat capacity of water is 4.18 J/g°C)

How much heat, in kJ, is required to warm 1.59 L of water from 23.7 °C to 79.5 °C? The specific heat of water is 4.184 J/g°C. Assume a density of 1.00 g/mL for water.

How much would the temperature of 309 g of ethanol increase if 25.3 kJ of heat were added to it? The specific heat of ethanol is 2.42 J/g°C.