Question

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

Answer 1

Answer:

D. 313 kJ.

Explanation:

Hello!

In this case, since the latent heat of a substance is that heat it releases or absorbs during a phase transition among solid, liquid and gas phases, it is given that it is computed as shown below:

$Q=n*\Delta H_{change}$

Whereas n are the moles of the substance and the ΔH of change is referred to freezing, melting, condensation, vaporization, sublimation or deposition; therefore, for the vaporization of those gien 7.72 mol of liquid water we obtain:

$Q=7.72mol*40.6kJ/mol\\\\Q=313kJ$

So the answer is D. 313 kJ.

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