Suppose 1g of water at 10 °C was heated and there are no heat lost in the surroundings. How much heat is needed to convert this amount of water to steam at 110 °C?

Calculate the amount of energy (in kJ) necessary to convert 497 g of liquid water from 0°C to water vapor at 182°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g °C, and for steam is 1.99 J/g °C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) kJ

Calculate the amount of heat (in kilojoules) required to convert 28.00 g of water to steam at 100 ° C. The enthalpy of vaporization for water is 40.79 kJ/mol.

The temperature of 1.9 kg of water is 100.0°C, but the water is not boiling, because the external pressure acting on the water surface is 3.0 x 105 Pa. Using the vapor pressure curve for water given in the figure, determine the amount of heat that must be added to the water to bring it to the point where it just begins to boil. Pressure, Pa 4 x 105 3 x 105 2 x 105- 1.01 x 105 0.53 x 105 0 50 50 83 100 Temperature, C 100 °C 150 1.01 x 105 Pa 83 C 0.53 x 105 Pa