Chapter 11, Problem 11.20P

Interpretation Introduction

Interpretation:

Given the phase diagram of carbon dioxide. Predict the sign of entropy change when carbon dioxide is changed from solid to gas. Also, find the temperature at which carbon dioxide spontaneously sublime at $1atm$. Calculate the entropy change if enthalpy changes for $1mol$ of carbon dioxide at solid state is $26.1kJ$.

Concept Introduction: Entropy can be defined as the measure of disorder. Entropy change for any substance is given using below formula:

$\Delta S=\frac{\Delta H}{T}$
Where, $\Delta S$ = Entropy Change
$\Delta H$ =Enthalpy Change
$T$ = Temperature