Calculate the heat absorbed when 134.7 g of ice is heated from -19.8oC to 135.2oC.  Specific heat of ice        =          2.04 J/goC  Specific heat of water    =          4.184 J/goC  Specific heat of steam   =          1.996 J/goC  Heat of fusion               =          334 J/g  Heat of vaporization      =          2264 J/g

What amount of heat (in kJ) is required to convert 19.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g-°C; specific heat capacity of liquid = 1.58 J/g-°C; AHfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)

calculate the amount of heat in kilojoules needed to convert 95.65 grams of ice at 0.00 degree celcius to a gas.  The molar heat of fusion for ice is 6.02 kj/mol, the molar heat of vaporization is 40.6 kj/mol, and the specific heat of water is 4.184j/g degrees Celcius.

How many joules of heat energy are needed to heat 25.0 g of ice at -5.0°C to a final temperature of 40.0°C. Specific heat of ice = 2.1 J/g°C. Be sure to consider the state of H20 present at 40.0°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.

The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 3.17 g3.17 g of water boils at atmospheric pressure?

The following information is given for ethanol at 1 atm: Boiling point = 78.40°C Melting point =-114.5°C Specific heat gas = 0.3418 cal/g°C Specific heat liquid = 0.5880 cal/g°C Heat of vaporization = 200.0 cal/g Heat of fusion = 26.04 cal/g A 44.00 g sample of liquid ethanol is initially at -58.80°C. How many kcal of energy must be added to the sample to raise its temperature to 94.90°C? Energy added = kcal

Under normal atmospheric pressure, nitrogen boils (and condenses) at - 196°C. When 7.7 g of nitrogen gas at -196°C was put into a dewar flask nitially at -260°C, their temperatures reach -210°C. If the specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-°C and 200 J/g, espectively, determine the heat capacity of the dewar flask.

Calculate the heat required to convert 22.2 g of propyl alcohol, C3H3O, from a solid at -141°C into the gaseous state at 115°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.

How much energy is needed to convert 59.5 grams of ice at 0.00 celsius to water at 60.9 celsius? specific heat(ice) = 2.10 J/g specific heat (water) 4.18 J/g heat of fusion= 6.02 kJ/mol heat of vaporization= 40.6 kJ/mol