Final answer:
The energy released when 6.0 g of water condenses from water vapor is calculated by first converting the mass of water to moles and then multiplying by the latent heat of vaporization of water, which is 40.7 kJ/mol. The correct calculation is 6.0 g x 1 mol/18.02 g x 40.65 kJ/mol.
Step-by-step explanation:
The amount of energy released when 6.0 g of water is condensed from water vapor can be calculated using the latent heat of vaporization of water. The heat of vaporization is the amount of energy required to convert one mole of a substance from a liquid to a gas (or vice versa) at constant temperature and pressure. In the case of water, it is 40.7 kJ/mol for condensation. To calculate the energy release for 6.0 g of water, we first convert the mass of water to moles by dividing by the molar mass of water (18.02 g/mol), and then multiply by the heat of vaporization:
Energy release = (Mass of water in g) x (1 mole/18.02 g) x (Heat of vaporization in kJ/mol)
Energy release = 6.0 g x (1 mol/18.02 g) x 40.7 kJ/mol
Thus, the correct answer is B. 6.0 g x 1 mol/18.02 g x 40.65 kJ/mol.