We're being asked to determine the characteristics for the standard electrochemical cell is tested with a voltmeter and it reads +0.035 volts.

*Recall that the greater the E**° _{cell} of a redox reaction, the more likely the reaction will occur (more spontaneous reaction)*

**E****°**_{cell}** > 0** → spontaneous in the forward direction**E****°**_{cell}** < 0** → nonspontaneous in the forward direction

**We have two ways (equations) of calculating the Gibbs Free Energy ΔG°:**

**Equation 1:**

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{\xb0}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}}$

A given standard electrochemical cell is tested with a voltmeter and it reads +0.035 volts. Having a good knowledge of chemistry, you immediately are thinking that the associated redox reaction has which of the following characteristics?

A. ∆G° is zero and K is equal to 1.

B ∆G° is positive and K is greater than 1.

C. ∆G° is negative and K is less than 1.

D. ∆G° is positive and K is less than 1.

E. ∆G° is negative and K is greater than 1.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.