A cell is made of two zinc rods. One dips into 0.014 mol/L zinc sulphate solution and the other…

Step 1. The anode. The dilute side makes more ions: $\text{Zn} \rightarrow \text{Zn}^{2+} + 2e^-$. The $0.014\ \text{mol/L}$ rod is the anode. Electrons go through the wire from that rod to the $0.84\ \text{mol/L}$ rod.

Step 2. The ratio. $\dfrac{0.84}{0.014} = 60$, and $\log 60 = 1.778$.

Step 3. The emf. $E = \dfrac{0.0591\ \text{V}}{2} \times 1.778 = 0.0525\ \text{V}$.

Step 4. Running down. The dilute solution gains $\text{Zn}^{2+}$ and the strong one loses it. The ratio falls towards 1. The cell stops when both solutions have the same concentration, and then $E = 0$.