a) ΔGº= -49,9 KJ/mol = - 50 KJ/mol)
b) The reaction goes to the right to the formation of products.
c) ΔG= 84,42 KJ/mol. The direction is too reactive, to the left to achieve equilibrium.
a) ΔGº= - RTLnKf
You need to convert Cº to K.
25ºC=298K
Then,
ΔGº = - 3,814 J/molK * 298K* Ln(5.6 10^8)
ΔGº = - 49906 J/mol
ΔGº = -49,9 KJ/mol
ΔGº = - 50 KJ/molb)
b) When the reactant and products are in their standard state, the direct reaction is spontaneous (the Go 0). In other words, the reaction proceeds to the right and results in the production of products.
c) The general equation for a chemical reaction is
aA + bB → cD + dD.
Thus
ΔG=ΔGº + RTLn (([C]^c[D]^d)/[A]^a*[B]^b)I
n this case,
ΔG = ΔGº + RTLn ([Ni(NH3)62+] / [Ni2+]*[NH3]^6 )
ΔG = 84417 J/mol
ΔG =84,42 KJ/mol
The reaction is not spontaneously occurring in the direction of the products if G > 0. Consequently, the movement is too reactive and to the left.
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The complete question is:
Ni2+(aq) + 6 NH3(aq) ⇌ Ni(NH3)6 2+(aq)
is Kf = 5.6 × 108 at 25°C.
(a) What is ΔG o
at this temperature?
(b) If standard-state concentrations of reactants and products are mixed, in which direction does the reaction proceed?
(c) 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?
