Respuesta :
The value of Δ[tex]S^{o}[/tex] for the surrounding when 2.41 moles of [tex]H_{2}[/tex] gas react at standard condition is 48.2 J/K.
What is entropy change and how to calculate it for the given equation?
Entropy change can be defined as the difference between the entropies of all the reactants and products multiplied by the corresponding number of moles for each.
Δ[tex]S_{rxn}[/tex] = Σ(n × [tex]S_{product}[/tex]) - Σ(n × [tex]S_{reactant}[/tex])
where, n = number of moles
For the given reaction:
[tex]H_{2}[/tex](g) + [tex]Cl_{2}[/tex](g) = [tex]2HCl[/tex](g)
The standard absolute entropies (S) are:
[tex]H_{2}[/tex] = 131 J/K .mole
[tex]Cl_{2}[/tex] = 223 J/K .mole
[tex]HCl[/tex] = 187 J/K .mole
On putting these values in above equation for calculating entropy change:
Δ[tex]S_{rxn}[/tex] = 2 × 187 - (131 + 223)
Δ[tex]S_{rxn}[/tex] = 374−131−223 = 20 J/K .mole
Entropy change of the surroundings when 1 mole of [tex]H_{2}[/tex] reacts = 20 J/K .mole
Now, when 2.41 moles of [tex]H_{2}[/tex] react, the entropy change of surrounding can be calculated as = 20 × 2.41 = 48.2 J/K
Therefore, the value of Δ[tex]S^{o}[/tex] when given moles of [tex]H_{2}[/tex] react is 48.2 J/K.
To know more about entropy change problems, visit:
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