Answer:
0.429 L of water
Explanation:
First to all, you are not putting the value of the energy given to vaporize water, so, to explain better this problem, I will assume a value of energy that I took in a similar exercise before, which is 970 kJ.
Now, assuming that the water density is 1 g/mL, this is the same as saying that 1 g of water = 1 mL of water
If this is true, then, we can assume that 1 kg of water = 1 L of water.
Knowing this, we have to use the expression to get energy which is:
Q = m * ΔH
Solving for m:
m = Q / ΔH
Now "m" is the mass, but in this case, the mass of water is the same as the volume, so it's not neccesary to do a unit conversion.
Before we begin with the calculation, we need to put the enthalpy of vaporization in the correct units, which would be in grams. To do that, we need the molar mass of water:
MM = 18 g/mol
The enthalpy in mass:
ΔH = 40.7 kJ/mol / 18 g/mol = 2.261 kJ/g
Finally, solving for m:
m = 970 / 2.261 = 429 g
Converting this into volume:
429 g = 429 mL
429 / 1000 = 0.429 L of water
= 