The molar entropy, S^∘, of HCl at 298 K is 186.9 JK^-1 mol^-1 . Find S^∘(350 K) if CP(298-350 K)

step 1 The equation we are given an equation which states H2 in gaseous form plus CL2 in gaseous form f

The molar entropy, S^∘, of HCl at 298 K is 186.9 JK^-1...

The molar entropy, $S^{\circ},$ of $\mathrm{HCl}$ at $298 \mathrm{K}$ is $186.9 \mathrm{JK}^{-1} \mathrm{mol}^{-1} .$ Find $S^{\circ}(350 \mathrm{K})$ if
$C_{P}(298-350 \mathrm{K})$ is $29.1 \mathrm{JK}^{-1} \mathrm{mol}^{-1}$.

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Key Concepts

Temperature Dependence of Entropy

The change in entropy with temperature can be determined by integrating the heat capacity over a specified temperature range. Under the assumption of constant heat capacity, the entropy change is calculated using the expression ?S = C? ln(T?/T?). This relationship links temperature change and the corresponding increase in molecular disorder, which is central to understanding thermodynamic processes.

Molar Entropy

Molar entropy is a thermodynamic property that measures the amount of disorder or randomness per mole in a substance. It is expressed in joules per kelvin per mole (J K?¹ mol?¹) and is fundamental in determining the spontaneity of chemical processes and assessing the energy dispersal within a system.

Heat Capacity at Constant Pressure

Heat capacity at constant pressure (C?) is a measure of the amount of heat required to raise the temperature of one mole of a substance by one kelvin while maintaining constant pressure. It plays a significant role in evaluating how the entropy of a substance changes with temperature because it defines the energy absorbed as thermal motion increases.

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