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I agree with all the previous responses, and it makes sense if you think about the meaning of these values. Ecell can describe spontaneity (spontaneous if the value is positive, not spontaneous if the value is negative) while K, the equilibrium constant, describes whether the reaction is product or reactant favored. We can see that spontaneous reactions will have more product (Ecell>0 and K>1) while nonspontaneous reactions will have more reactants (Ecell<0 and K<1).
Looking at the two equations E˚= (RT/nF)lnK and Ecell = E˚- (RT/nF)lnQ, you can see that if K>1 then E˚> 0. When E˚>0, then Ecell will be a greater value and will most likely be greater than zero as well. So if K>0 then E˚>0 and Ecell>0.
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