How much heat (in kJ) would be required to convert 21.0 g of ice to water at 0°C?

How many joules of energy must be removed from 152 g of water at 18.5 °C to form ice at 0 °C?

If we start with 10g of ice at -5°C and heat it until we have liquid water at 45°C, how much heat energy will be needed (kJ)?     The specific heat of ice is 2.03J/g°C and the specific heat of liquid water is 4.18J/g°C.     ΔHfusion is 334 J/g.

What amount of heat energy (in Joules) is needed to completely melt 5.4 grams of sucrose (C12H22O11) that is at 37°C?

You pour 84 mL of 1.5 M HNO3 and 284 mL of 0.50 M KOH over 50 g ice. The solutions and the ice were both initially at 0C. How much ice melts? Assume the heat of neutralization is -57.3 kJ/mol.

What quantity of heat (in KJ) would be required to convert 11.1 g of ice to water 0.00 C ? (Hfus=6.01 KJ/ mol for water)

What quantity of heat (in kJ) would be required to convert 15.1 g of ice to water at 0.00°C? (AHfus = 6.01 kJ/mol for water)

How much heat must be added to 100 g of ice at -5°C to turn it into 60 grams of water and 40 grams of steam, both at 100°C? Cp H2O = 75.7 J/mol-K, Cp Ice = 37.7 J/mol-K, Cp Steam = 35.1 J/mol-K, ΔHfus = 6.01 kJ/mol, ΔHvap = 40.7 kJ/mol

Which equation calculates the heat of vaporization of water when it takes the same amount of heat to boil 5 g of water as it does to heat 100 g of water by 27°C?   Question 11 options:   (100 g × 4.184 J g–1 °C–1 × 27°C)  / (5 g / 18 g mol–1)   (5 g × 4.184 J g–1 °C–1 × 27°C)  / (100 g / 18 g mol–1)   (5 g / 18 g mol–1) / (100 g × 4.184 J g–1 °C–1 × 27°C)

How much heat (in kJ) would be required to convert 29.4 g of ice to water at 0.00°C? (∆Hfus = 6.01 kJ/mol for water)