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A silver half-cell has E° = +0.80 V and an iron half-cell has E° = -0.44 V…

Try it on paper first. A hint, the key idea and the worked solution are here when you need them.

A silver half-cell has $E^\circ = +0.80\ \text{V}$ and an iron half-cell has $E^\circ = -0.44\ \text{V}$ . They are joined to make a cell. Say which is the cathode and find the cell potential.

Need a reminder? The key ideaShow

$E^\circ$ is a reduction potential, measured against the standard hydrogen electrode, which is $0.00\ \text{V}$ , at $1\ \text{mol/L}$ , $1\ \text{bar}$ and $298\ \text{K}$ . $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}$ . Reversing a half-reaction changes the sign of $E^\circ$ . Multiplying it changes nothing.

The worked solution

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Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.

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