The molar heat of vaporization of water at 25 °C is +43.9 kJ/mol. How many kilojoules of heat would be required to vaporize 8.82 g of 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

The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 1.59 g of water boils at atmospheric pressure?.

Calculate the heat released when 65.5g of water at 55.5 ° C cools to ice at 0.0 ° C. (Given that the specific heat of liquid water is 1.00 calg×°C, and heat of water solidification is 80.0 cal/g.).

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)

4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C? 5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to steam at 105.0 °C. How much heat would be released in the reverse process?

How much heat is required to vaporize 30 g of water at 100˚C?

How much heat is required to convert 20.0 g of ice at -50.0 degrees Celcius to liquid water at 0.0 degrees Celcius?