Question

The value of ΔG∘ at 221.0∘C for the formation of phosphorous
trichloride from its constituent elements,

P2(g)+3Cl2(g)→2PCl3(g)

is ________ kJ/mol. At 25.0∘C for this reaction, ΔH∘ is
−720.5kJ/mol, ΔG∘ is −642.9kJ/mol, and ΔS∘ is −263.7J/K.

Answer #1

From Gibbs free energy relationship, we have

ΔG^{∘} = ΔH^{∘} - TΔS^{∘}

given T= 221.0^{o}C = 221 + 273.15 = 494.15 K

ΔG^{∘} = ΔH^{∘} - TΔS^{∘} = −720.5
kJ/mol - [ 494.15 K x −263.7 J/K],

but ΔS^{∘} value is in J/K convert it into kJ/K as 1 kJ
= 100J

assume ΔH^{∘} and ΔS^{∘} values are independent
over the temperature change.

ΔG^{∘} = ΔH^{∘} - TΔS^{∘} = −720.5
kJ/mol - [ 494.15 K x −0.2637 kJ/K]

ΔG^{∘} = -590.192645 kJ/mol

**ΔG ^{∘} = -590.2 kJ/ mol
-------------- Your Answer with 4 sig fig (Please note that
negative sign before value)**

**Thank You So Much! Please Rate this answer as you
wish.**

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enthalpy change for the formation of one mole of substance from its
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values can be used to calculate the enthalpy change of any
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Consider, for example, the reaction
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ΔH∘f
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