Question

E. Compare the entropy of the

H₂O(l) to the H₂O(g) that is formed

F. Determine the mass of liquid water that vaporizes if 7700 joules of energy is absorbed by the H₂O(l) at 100.°C.

Answer 1

e. The entropy of the H₂O(g) is greater than that of H₂O(l) because gases have more entropy than liquids.

f. We need to use the formula:

q = m × ΔHvap

where q is the heat absorbed, m is the mass of liquid water that vaporizes, and ΔHvap is the enthalpy of vaporization of water (40.7 kJ/mol or 2257 J/g at 100°C).

To use this formula, we need to convert the given energy of 7700 J to kJ:

7700 J ÷ 1000 = 7.7 kJ

Then, we can plug in the values:

7.7 kJ = m × 2257 J/g

m = 7.7 kJ ÷ 2257 J/g

m = 3.41 g

Therefore, 3.41 g of liquid water would vaporize if 7700 J of energy is absorbed by the H₂O(l) at 100°C.

Step-by-step explanation:

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