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.

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.)

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 do you calculate the heat change when a solute with known mass is dissolved in water, considering its lattice energy and heat of hydration?

If a hot metal with a mass of 5.21 grams undergoes a temperature decrease of 18.18 °C and releases 150 J of heat, what is the specific heat capacity of the metal?

Suppose that 0.44 g of water at 25 °C condenses on the surface of a 51-g block of aluminum that is initially at 25 °C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in °C)?

In a process where 4.80 kg of boiling water is used to raise the temperature of 25.0 kg of water in a bath to body temperature, how much heat is transferred if the heat lost by the boiling water is equal to the heat gained by the room-temperature water?