Question

In: Chemistry

For a particular reaction at 129.9 °C, ΔG = 319.61 kJ/mol, and ΔS = 777.00 J/(mol·K)....

For a particular reaction at 129.9 °C, ΔG = 319.61 kJ/mol, and ΔS = 777.00 J/(mol·K). delta g is -47.6 celcius

Expert Solution

T = 129.9 + 273 = 402.9 K

ΔG = 319.61 kJ/mol

ΔG = - RT ln K

319.61 = -8.314 x 10^-3 x 402.9 x ln K

lnK = -95.41

K = 3.66 x 10^-42

ΔS = 777.00 J/(mol·K)

= 0.777 kJ / mol K

ΔG = ΔH - T ΔS

319.61 = ΔH - 402.9 x 0.777

ΔH = 632.66 kJ / mol K

now :

T2 = 402.9 K

K2 = 3.66 x 10^-42

T1 = -47.6+273 = 225.4 K

K1 = ?

ln (K2 / K1) = ΔH / R ) [1/T1 - 1/T2]

ln (3.66 x 10^-42 / K1 ) = 632.66 / (8.314 x 10^-3) [1/225.4 - 1/402.9]

= 148.73

K1 = 9.36 x 10^-107

ΔG = - RT ln K

ΔG = -8.314 x 10^-3 x 225.4 x ln (9.36 x 10^-107)

ΔG = 457.51 kJ / mol

queen_honey_blossom answered 2 years ago

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