A mass of 0.063 kg of water was turned into steam.The specific latent heat of vaporisation of water is 2 260 000 J/kgCalculate the thermal energy transferred to the water to turn it into steam.Use the equation:thermal energy for a change of state = mass ×specific latent heatEnergy = ___________________________ J

1000kg of steam is condensed back to water in the condenser of a power station each hour. The specific latent heat of vaporisation of water is 2260kJ/kg.Calculate the energy output to the environment this causes each second.

(f)     While a kettle boils, 0.018 kg of water changes to steam.Calculate the amount of energy required for this change.Specific latent heat of vaporisation of water = 2.3 × 10 6 J / kg.

The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is released when 5.00 g of steam condenses to liquid water at 100°C. Hint: Convert 5.0 grams of water to moles (divide by the molar mass of H2O), multiply answer by the heat of vaporization.

1695 kJ of energy is transferred to water at 100 °CThe specific latent heat of vaporisation of water is 2.260 × 10 6 J / kgCalculate the mass of water changed into a gas at 100 °CEnergy transferred = mass x specific latent heat

2. 650g of water at 100 ∘ C is boiled continuously. If the latent heat of vaporisation of water is 2260000J/kg, how much energy is needed to boil the water? Assume that no temperature change occurs.Give your answer to three significant figures.