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

D. 313 kJ.

Step-by-step 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.

Best regards!