Chapter 5, Problem 5.35NP

Interpretation Introduction

Interpretation:

Between 0⁰C and 100⁰C, the heat capacity of Hg(I) is given by $\text{CP,m }\left(\text{Hg,I}\right){\text{ J}}^{\text{-1}}{\text{K}}^{\text{-mol}}\text{= 30}\text{.093 – 4}\text{.944 }\times {\text{ 10}}^{\text{-3}}\text{TK}$ . The value of $\text{ΔΗ and ΔS}$ needs to be calculated, if 2.25 moles of Hg(I) are raised in temperature from 0.00⁰C to 88.0⁰C at constant P.

Concept Introduction :

Enthalpy is known as the sum of internal energy and product of pressure andvolume provided by the below equation:

  $H=U+PV$ .

When the procedure happens at constant pressure, the evolved heat is equal to the change in enthalpy.

The entropy of a system can’t increase in a reversible adiabatic procedure.