The following electrochemical cell has been set up.
`Pt(1) |Fe^(3+) , Fe^(2+) (a =1) || Ce^(4+), Ce^(3+) (a = 1) | Pt(2)`
`E^@ (Fe6(3+) // Fe^(2+) ) = 0.77V , E^@ (Ce^(4+) // Ce^(3+)) = 1.61 V`
If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current. Will the current increase or decrease with time?

Explanation

To solve the problem, we need to analyze the electrochemical cell and determine the direction of current flow as well as whether the current will increase or decrease over time.

### Step-by-Step Solution:

1. **Identify the Half-Reactions**:
- The cell consists of two half-reactions:
- **Oxidation**: \( \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + e^- \) (This occurs at the anode)
- **Reduction**: \( \text{Ce}^{4+} + e^- \rightarrow \text{Ce}^{3+} \) (This occurs at the cathode)
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