Determine δg when [ni(nh3)62+] = 0.010 m, [ni2+] = 0.0010 m, and [nh3] = 0.0050 m. in which direction will the reaction proceed to achieve equilibrium? ni2+(aq) + 6 nh3(aq) ⇌ ni(nh3)6 2+(aq) is kf = 5.6 × 108 at 25°

Given:

The reaction is

We know that

Δ

Δ

Δ

For the given reaction the reaction quotient will be :

Q = \frac{[Ni(NH_{3} )_{6} ^{+2}] }{[Ni^{+2} ][NH_{3}]^{6}

On putting values

Q  will be equal to =

The relation between standard and other free energy change is

ΔG = Δ

Thus

ΔG = (-49906.8) + (8.314)(298) ( ln ()

ΔG = (-49906.8) + 84466

ΔG = 34535 J / mol K

ΔG  is positive so reaction is not spontaneous in forward direction

It will proceed in reverse direction, it will move from product to reactant

12 is it do you think so