Answer:
a. ΔG⁰ = -49.9 kJ/mol
b. The reaction proceeds towards right direction
c. ΔG = 49.5 kJ/mol
d. The reaction proceeds towards left direction
Explanation:
a. It is possible to obtain ΔG⁰ from K reaction using:
ΔG⁰ = -RT ln K
<em>Where R is gas constant 8.314 J/molK, T is absolute temperature (273.15 +25 = 298.15K)</em>
Replacing:
ΔG⁰ = -8.314 J/molK 298.15K ln 5.6x10⁸
<em>ΔG⁰ = -49.9 kJ/mol</em>
b. Reaction quotient Q, defines concentrations of substances involved in an equilibrium, when Q = Kf, the reaction is in equilibrium, when Q < Kf the reaction moves towards right direction and vice versa.
At standard-state concentrations, Q = 1, as:
Q < Kf, <em>the reaction proceeds towards right direction</em>
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c. ΔG = ΔG⁰ + RT ln Q
Q = [Ni(NH₃)₆²⁺] / [NH₃]⁶[Ni²⁺]
Q = 0.017M / 0.0015M⁶×0.0058M
Q = 2.6x10¹⁷
ΔG = -49.9 kJ/mol + 8.314x10⁻³ kJ/molK 298.15K ln 2.6x10¹⁷
<em>ΔG = 49.5 kJ/mol</em>
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d. As Q > Kf, <em>the reaction proceeds towards left direction</em>
