The specific heat capacity of liquid ammonia is 4700J/Kg.K and its latent heat of vaporization is 1370 kJ/kg. Determine the amount of thermal energy needed to raise the temperature of 1750 g of liquid ammonia from -70.0° C to its boiling point, -33.5° C, and then vaporize it completely.

Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.

From the molar heats of formation in Appendix G, determine how much heat is required to evaporate one mole of water: H2O(l)H2O(g)

1. Which of the following processes requires the largest input of energy as heat? raising the temperature of 100 g of water by 1.0 °C vaporization of 0.10 g of water at 100 °C melting 1.0 g of ice at 0 °C warming 1.0 g of ice from −50 °C to 0 °C (specific heat of ice = 2.06 J/g · K)

The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.

Which requires the absorption of a greater amount of heat—vaporizing 100.0 g of benzene or boiling 20.0 g of water? (Use Table 8.2.)

Explain why the enthalpies of vaporization of the following substances increase in the order CH4NH3H2O, even though all three substances have approximately the same molar mass.

A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0C. The reaction is 2Na(s)+2H2O(l)2NaOH(aq)+H2(g)H=368kJ Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/gc, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.

Follow the step-wise process outlined in Problem 31 to calculate the amount of heat involved in condensing 100.00 g of benzene gas (C6H6) at 80.00C to liquid benzene at 25.00C. Use Tables 8.1 and 8.2 for the specific heat, boiling point, and heat of vaporization of benzene.

Will a closed container of water at 70 C or an open container of water at the same temperature cool faster on a cold winter day? Explain why.