Consider the generic reaction below:
A (aq) + 2 B (aq) ⇌ C (aq) + D (aq)
Where ΔGo is -10.2 kJ for the reaction
True False If the reaction shown is at equilibrium,
ΔGo is equal to zero
True False Under certain conditions
ΔGnonstandard is negative, the value of
ΔGnonstandard is the amount of energy free to do work
under those conditions
True False This reaction will always be spontaneous
because ΔGo is negative
True False ΔGnonstandard allows us to
determine the equilibrium constant, K, for the reaction
1) If the reaction shown is at equilibrium, ΔGo is equal to zero ( TRUE)
reason :
if ΔGo is equal to zero ΔGo = - R T ln K
K = 1 . equilibrium constant is equal to 1 at equilibrium
2) Under certain conditions ΔGnonstandard is negative, the value of ΔGnonstandard is the amount of energy free to do work under those conditions (True)
3) This reaction will always be spontaneous because ΔGo is negative (TRUE)
reason : for spontaneous reaction ΔGo is negative
4) ΔGnonstandard allows us to determine the equilibrium constant, K, for the reaction ( False )
reason : because equilibrium constant is determined by ΔGo but not ΔGnonstandard
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