Chapter 17, Problem 17.32CP

Interpretation Introduction

Interpretation:

The signs $\left(+,-,0\right)$ of $\Delta H,\Delta Sand\Delta G$ for the process should be explained

Concept Introduction:

• Isothermal process: - If the temperature of the system remains constant during the change and heat is exchanged between the system and surrounding such processes are called isothermal process.
• Enthalpy $\left(\Delta H\right)$:- It is defined as the sum of internal energy and the pressure-volume energy of the system.
  $\Delta H=\Delta U+P\Delta V$
• Internal energy $(\Delta U)$:-It is equal to the sum of heat supplied to the system and work done on the system.
  $\Delta U=q+w$
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• Entropy $\left(\Delta S\right)$:-It is defined as a measure of the disorder or randomness of the system. More the randomness, more is the entropy.
  $\Delta S=\frac{q}{\Delta T}$
• Gibb’s free energy $\left(\Delta G\right)$:- It is the amount of energy available from a system that can be converted into useful work. It is a measure of its capacity to do useful work.
  $\Delta G=\Delta H-T\Delta S$

To explain: The sign of $\Delta H,\Delta Sand\Delta G$ for the process.