How much energy is released when 2.05 mol of water vapour at 100C condenses with no change in temperature?
Q=-83.4 KJ
Ur welcome😌
Well, let me put on my comedic goggles and calculate that for you! To calculate the energy released when 2.05 mol of water vapor condenses, we need to use the molar enthalpy of vaporization for water. But hey, who wants to turn into a human calculator? Not me! So, here's a joke instead:
Why don't scientists trust atoms?
Because they make up everything!
But seriously, to answer your question, the molar enthalpy of vaporization for water is approximately 40.7 kJ/mol. So, when 2.05 mol of water vapor condenses, we can calculate the energy released:
Energy released = (2.05 mol) * (40.7 kJ/mol)
Punching that into the calculator, we find:
Energy released ≈ 83.435 kJ
So, approximately 83.435 kJ of energy is released when 2.05 mol of water vapor condenses. I hope that provides you with a refreshing answer!
To calculate the energy released when 2.05 mol of water vapor at 100°C condenses, we need to use the heat of vaporization of water. The heat of vaporization is the amount of energy required to convert 1 mole of water from its liquid phase to its vapor phase at the same temperature.
The heat of vaporization of water is approximately 40.7 kJ/mol. This means that 40.7 kJ of energy is required to convert 1 mole of water from a liquid to a vapor at 100°C.
Since we want to calculate the energy released when 2.05 mol of water vapor condenses, we need to multiply the heat of vaporization by the number of moles:
Energy released = Number of moles x Heat of vaporization
Energy released = 2.05 mol x 40.7 kJ/mol
Energy released = 83.435 kJ
Therefore, when 2.05 mol of water vapor at 100°C condenses with no change in temperature, approximately 83.435 kJ of energy is released.
To calculate the amount of energy released when water vapor condenses, we need to use the formula for enthalpy change. The enthalpy change during a phase change can be calculated using the equation:
ΔH = n × ΔHv
Where:
ΔH is the enthalpy change
n is the amount of substance (in moles)
ΔHv is the molar heat of vaporization
The molar heat of vaporization for water is approximately 40.7 kJ/mol. However, since the question involves the condensation of water, which is the reverse process, we need to use the negative of the molar heat of vaporization.
Therefore, the value of ΔHv for the condensation of water is -40.7 kJ/mol.
Now, let's calculate the energy released when 2.05 mol of water vapor condenses:
ΔH = n × ΔHv
ΔH = 2.05 mol × (-40.7 kJ/mol)
ΔH = -83.435 kJ
Therefore, when 2.05 mol of water vapor at 100°C condenses with no change in temperature, approximately 83.435 kJ of energy is released.