A cell has E^°cathode = +0.34 V and E^°anode = -0.76 V. Compute the standard cell potential in volts.

Practice question · Numerical answer

A cell has $E^\circ_{cathode} = +0.34$ V and $E^\circ_{anode} = -0.76$ V. Compute the standard cell potential in volts.

Hints

Cell potential is cathode minus anode.
Compute 0.34 - (-0.76).

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Why

$E^\circ_{cell} = 0.34 - (-0.76) = +1.10$ V. This is the Daniell cell of zinc and copper, and the positive value confirms the reaction is spontaneous as written.

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A cell has Ecathode∘=+0.34E^\circ_{cathode} = +0.34Ecathode∘​=+0.34 V and Eanode∘=−0.76E^\circ_{anode} = -0.76Eanode∘​=−0.76 V. Compute the standard cell potential in volts.

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A cell has $E^\circ_{cathode} = +0.34$ V and $E^\circ_{anode} = -0.76$ V. Compute the standard cell potential in volts.