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Vedmedyk [2.9K]
2 years ago
12

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 -720.5 kJ/mol, ΔG° is -642.9 kJ/mol, and ΔS° is -263.7 J/K.
Chemistry
1 answer:
densk [106]2 years ago
3 0

Answer:

ΔG    = - 590.20 kJ/mol

Explanation:

The formula for calculating Gibb's Free Energy  can be written as:

ΔG    =    ΔH - TΔS

Given That:

ΔH = -720.5 kJ/mol

T = 221.0°C = (221.0 + 273.15) = 494.15 K

ΔS° = -263.7 J/K

So; ΔS° = -0.2637 kJ/K if being converted from joule to Kilo-joule

Since we are all set, let replace our given data in the above equation:

ΔG    =  (-720.5 kJ/mol) - (494.15 K) ( - 0.2637 kJ/K)

ΔG    =  (-720.5 kJ/mol) - (- 130.30755)

ΔG    =  -720.5 kJ/mol + 130.30755

ΔG    =  -590.192645 kJ/mol

ΔG    = - 590.20 kJ/mol

Thus, 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 <u>-590.20</u> kJ/mol.

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