1. Tardigrade
  2. Question
  3. Chemistry
  4. Given the following entropy values (in J K-1 mol-1) at 298 K and 1 atm: H2(g): 130.6, Cl2(g): 223.0, HCl(g): 186.7 .The entropy change (in J K-1 mol-1) for the reaction H2 (g) + Cl2 (g) arrow 2HCl (g) is

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Q. Given the following entropy values (in $J \, K^{-1} \, mol^{-1}$) at $298 \,K$ and $1$ atm : $H_{2}(g) : 130.6, Cl_{2}(g) : 223.0, HCl(g) : 186.7$ .The entropy change (in $J \, K^{-1} mol^{-1}$) for the reaction
$H_{2} (g) + Cl_{2 } (g) \rightarrow 2HCl (g)$ is

Thermodynamics

Solution:

Entropy change
$\Delta S = \Delta S_{\text{product}} - \Delta S_{\text{reactant}}$
$= 2 (186.7) - (223 + 130.6) $
$= 373.4 - 353.6$
$ = 19.8 \, JK^{-1} \, mol^{-1}$