What is the answer and how do I Calculate the quantity of energy required to change 3.00 mol of liquid water to steam at 100°C. The molar heat of vaporization of water is 40.6 kJ/mol.
Wouldnt the heat = Hv*number of moles?
To calculate the quantity of energy required to change 3.00 mol of water to steam at 100°C, you can use the equation:
Energy = n * ΔHvap
Where:
- Energy is the quantity of energy required
- n is the number of moles of water
- ΔHvap is the molar heat of vaporization of water
In this case, you have n = 3.00 mol and ΔHvap = 40.6 kJ/mol.
To calculate the energy, you can substitute these values into the equation:
Energy = 3.00 mol * 40.6 kJ/mol
Multiply the number of moles (n) by the molar heat of vaporization (ΔHvap) to get the answer.