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.
Question
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.
Solution
Sure, here are the steps to calculate the quantity of heat released:
-
First, we need to convert the mass of water to moles. The molar mass of water (H2O) is approximately 18.015 g/mol. So, we divide the given mass of water by the molar mass of water:
5.00 g / 18.015 g/mol = 0.277 moles
-
Next, we multiply the number of moles by the heat of vaporization to find the total heat released. The heat of vaporization is the amount of heat required to convert one mole of a substance from a liquid state to a gaseous state at a constant temperature and pressure. In this case, it's given as 40.66 kJ/mol. So:
0.277 moles * 40.66 kJ/mol = 11.27 kJ
So, the quantity of heat that is released when 5.00 g of steam condenses to liquid water at 100°C is approximately 11.27 kJ.
Similar Questions
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
0.595 g sample of steam at 107.4∘C is condensed into a container with 5.77g of water at 16.5∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 J g⋅∘C, the specific heat of steam is 2.01 Jg⋅∘C, and Δ𝐻vap=40.7 kJ/mol.
Latent heat of vaporisation of water is 540 cal g–1 at 100°C. Calculate the entropy change when 1000 g water is converted to steam at 100°C. :- 1447 cal2447 cal3447 cal4447 cal
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.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.