If this energy were used to vaporize water at 100.0 ∘C, how much water (in liters) could be vaporized? The enthalpy of vaporization of water at 100.0 ∘C is 40.7 kJ⋅mol−1. (Assume the density of water is 1.00 g/mL.)

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

tallinn tallinn · Answer 2 · 2022-02-01T16:25:45+01:00

The correct answer is 0.429 L of water

When we are not putting the value of the energy given to vaporize water I will assume a value of energy that I took in a similar exercise before, which is 970 kJ.
Now, we are assuming that the water density is 1 g/mL, this is the same as saying that 1 g of water = 1 mL of water
Although when If this is true, then, we can assume that 1 kg of water = 1 L of water.

Now, we have to use the expression to get energy which is:

Then Q = m * ΔH
Solving for is m:
Now m = Q / ΔH

Now after that "m" is the mass, but in this case, the mass of water is the same as the volume, also that it's not necessary to do unit conversion.
Before that we begin with the calculation, then we need to put the enthalpy of vaporization in the correct units, also that which would be in grams. To do that, then we need the molar mass of water:

Then MM = 18 g/mol
The enthalpy in mass:
After that ΔH = 40.7 kJ/mol / 18 g/mol = 2.261 kJ/g
Finally, solving for m:
Then m = 970 / 2.261 = 429 g
Then Converting this into volume:
Now, 429 g = 429 mL
Thus, 429 / 1000 = 0.429 L of water

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