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For a spontaneous reaction, the $\Delta G$, equilibrium constant, K and $E^\circ _{cell}$ will be respectively

(a) -ve, > 1, +ve
(b) +ve, > 1, -ve
(c) -ve, < 1, -ve
(d) -ve, > 1, -ve
Can you answer this question?

1 Answer

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  • ∆ G= free energy, spontaneity
  • Negative: spontaneous
    Positive: non-spontaneous
    Equal to Zero: at equilibrium/ becomes K
  • ∆ G= ∆ H- T ∆ S, T being temp (Kelvin) (Relations of temperature: decrease in temp. = ∆ G is positive; increase in temp. = ∆ G is negative)
  • ∆G= -RT ln K R being gas constant= 8.3145 J/K*mol and K being equilibrium constant equation (equation only for concentration at equilibrium)
Answer: -ve, > 1, +ve
For a spontaneous reaction $\Delta G$ is -ve
$\Delta G = -nFE_{cell}$
or, ln K is +ve $\Rightarrow$ K > 1
Now, $\Delta G = -nFE_{cell}$
As, $\Delta G$ is -ve for a spontaneous reaction. $E_{cell}$ for such a reaction is +ve.
answered Feb 26, 2014 by mosymeow_1
edited Feb 26, 2014 by mosymeow_1

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