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2 years ago

The value of delta G at 141.0 degrees celsius for the formation of phosphorous trichloride from its constituent elements,

Chemistry

1 answer:

AURORKA [14]2 years ago

6 0

Answer:

The correct answer is option E.

Explanation:

The Gibbs free energy is given by expression:

ΔG = ΔH - TΔS

ΔH = Enthalpy change of the reaction

T = Temperature of the reaction

ΔS = Entropy change

We have :

ΔH = -720.5 kJ/mol = -720500 J/mol (1 kJ = 1000 J)

ΔS = -263.7 J/K

T = 141.0°C = 414.15 K

$\Delta G = -720500 J/mol - (414.15 K\times (-263.7 J/K))$

$= -611,288.64 J/mol = -611.28 kJ/mol\approx -611.3 kJ/mol$

The Gibb's free energy of the given reaction at 141.0°C is -611.3 kJ/mol.

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2 years ago

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$\large \boxed{\text{0.603 mol}}$

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2 years ago

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