Consider the reaction a + b c +

d. at biochemical equilibrium (25°c, ph of 7), the concentration of a is 0.2 m, the concentration of b is 0.2 m, the concentration of c is 0.8 m, and the concentration of d is 0.8 m. calculate δg and δg° ′ under these conditions.

Question

Julio Summers

Chemistry

27 August, 19:10

Consider the reaction a + b c +

d. at biochemical equilibrium (25°c, ph of 7), the concentration of a is 0.2 m, the concentration of b is 0.2 m, the concentration of c is 0.8 m, and the concentration of d is 0.8 m. calculate δg and δg° ′ under these conditions.

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Valeria · Answer 1

When the reaction is at equilibrium ∴ΔG = Zero

now we need to get Δ G°, we can get it from this formula:

ΔG° = - RT㏑K (eq)

when we have R = 8.315 J/mol°K and T in Kelvin = 25+273 = 298

so we need to get the K (eq) from this formula:

K (eq) = concentration of products / concentration of reactants

= [ C] [ D] / [A] [B]

= (0.8*0.8) / (0.2*0.2) = 16

by substitution in ΔG° formula:

∴ ΔG° = - 8.315 * 298 * ㏑ (16) = - 6870 Jmol^-1 / 1000 = - 6.87 KJ mol^-1

Consider the reaction a + b c +d. at biochemical equilibrium (25°c, ph of 7), the concentration of a is 0.2 m, the concentration of b is 0.2 m, the concentration of c is 0.8 m, and the concentration of d is 0.8 m. calculate δg and δg° ′ under these conditions.

Consider the reaction a + b c +

d. at biochemical equilibrium (25°c, ph of 7), the concentration of a is 0.2 m, the concentration of b is 0.2 m, the concentration of c is 0.8 m, and the concentration of d is 0.8 m. calculate δg and δg° ′ under these conditions.