Calculate the quantity of energy required to change 7.72 mol of liquid water to steam at 100^oC. The molar heat of vaporization of water is 40.6 kJ/mol. A) 5.26 kJ B) 40.6 kJ C) 313 kJ D) 77.2 kJ E) 48.3 kJ

Question

Quizplus · Accepted Answer

The quantity of energy required to change liquid water to steam can be calculated using the formula:
q = n * ΔHvap
where q is the quantity of energy required, n is the number of moles of water, and ΔHvap is the molar heat of vaporization.
Plugging in the values,
q = 7.72 mol * 40.6 kJ/mol
q = 313 kJ
Therefore, the answer is (C) 313 kJ.

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