How many faradays of electric charge is required to liberate `5600cm^(3)` of oxygen at STP?

Explanation

To determine how many Faradays of electric charge are required to liberate 5600 cm³ of oxygen at STP, we can follow these steps:

### Step 1: Understand the Reaction
The reaction for the liberation of oxygen can be represented as:
\[ 2 \text{H}_2\text{O} \rightarrow \text{O}_2 + 4 \text{H}^+ + 4 \text{e}^- \]
This indicates that to produce 1 mole of O₂, 4 moles of electrons (or 4 Faradays) are required.

### Step 2: Determine the Volume of Oxygen in Moles
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