To calculate the amount of energy involved in the condensation of steam to water, you need to use the equation for calculating the heat of vaporization. The heat of vaporization is the amount of energy required to turn a given amount of a substance from a liquid to a gas at a constant temperature.
For water, the heat of vaporization is approximately 40.7 kJ/mol. To calculate the energy involved in the condensation of 325 g of steam to water, you need to first convert the mass of the steam to moles using the molar mass of water, which is 18.015 g/mol.
Thus, 325 g of steam is equal to 325 g / 18.015 g/mol = 18.06 mol of water.
Using the heat of vaporization, the energy required to condense 18.06 mol of water from steam to a liquid at 100 degrees celsius is 18.06 mol * 40.7 kJ/mol = 735.9 kJ.
This is the amount of energy that must be removed in order to condense the steam to a liquid at 100 degrees celsius.