Chapter 2, Problem 2E.7E

Interpretation Introduction

Interpretation:

Thermodynamic state functions $q,w,\Delta Hand\Delta U$ when $2.50mol$ is vaporized at $250K$ and $750Torr$ has to be calculated.

Concept Introduction:

Heat of vaporization: At constant temperature and pressure, the amount of heat entails to convert a liquid into a gas. A gas produced same quantity of heat when it converts liquid.

Standard enthalpy change of reaction:

The standard enthalpy change of reaction is given by

  $\begin{array}{l}{\text{ΔH}}^{\text{o}}\text{=}{\displaystyle \sum {\text{nΔH}}_{\text{f}}^{\text{o}}}\left(\text{products}\right)\text{-}{\displaystyle \sum {\text{nΔH}}_{\text{f}}^{\text{o}}}\left(\text{reactants}\right)\\ \text{where,}\\ {\text{ΔH}}^{\text{o}}\text{-}\text{standard}\text{enthalpy}\text{change}\\ {\text{ΔH}}_{\text{f}}^{\text{o}}\text{-}\text{standard}\text{enthalpy}\text{change}\text{of}\text{formation}\end{array}$

Ideal gas Equation:

Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation.

  $\begin{array}{l}\text{V }\propto \frac{\text{nT}}{\text{P}}\\ \text{V = R}\frac{\text{nT}}{\text{P}}\\ \text{PV = nRT}\end{array}$       $\begin{array}{l}\text{where,}\\ \text{n = moles}\text{of}\text{gas}\\ \text{P = pressure}\\ \text{T = temperature}\\ \text{R = gas }\text{constant}\text{and }\text{V=}\text{Volume}\end{array}$