The standard molar heat of vaporization for water is 40.79 kJ/mol. How much energy
would be required to vaporize 4.00 mol of
water?
Answer in units of kJ
40.79 kJ/mol x 4.00 mol = ? kJ IF the temperature of the water is already at 100 C.
To calculate the energy required to vaporize 4.00 mol of water, we can use the molar heat of vaporization.
Given:
Standard molar heat of vaporization for water = 40.79 kJ/mol
Number of moles of water = 4.00 mol
To find the energy required to vaporize the water, we multiply the molar heat of vaporization by the number of moles:
Energy required = Standard molar heat of vaporization x Number of moles
Energy required = 40.79 kJ/mol x 4.00 mol
Energy required = 163.16 kJ
Therefore, the energy required to vaporize 4.00 mol of water is 163.16 kJ.
To find the amount of energy required to vaporize 4.00 mol of water, you can use the formula:
Energy = Standard molar heat of vaporization × Number of moles of water
Given:
Standard molar heat of vaporization = 40.79 kJ/mol
Number of moles of water = 4.00 mol
Substituting the values into the formula:
Energy = 40.79 kJ/mol × 4.00 mol
Multiplying the values:
Energy = 163.16 kJ
Therefore, the amount of energy required to vaporize 4.00 mol of water is 163.16 kJ.