Chapter 15, Problem 83A

sUse information from Figure 15.24 to calculate howmuch heat is required to vaporize 4.33 mol of waterat 100°C.

Interpretation Introduction

Interpretation: The heat of vaporization of water at 100⁰C needs to be determined.

Concept Introduction: The enthalpy of vaporization is the heat required to turn 1 mol liquid into vapour at boiling point.

Answer to Problem 83A

The heat required to vaporize 4.33 mol of water is 176.231 kJ.

Explanation of Solution

  $\begin{array}{l}\text{Heat required to vaporize 1 mol water(Δ}{H}_{\text{vap}}\text{)=40}\text{.7 kJ}\\ \text{Heat required to vaporize 4}\text{.33 mol water=40}\text{.7×4}\text{.33=176}\text{.231 kJ}\end{array}$

Conclusion

The heat required to vaporize 4.33 mol of water has been calculated.