The weight of silver (at `wt. = 108`) displaced by a quantity of electricity which displaced `5600 mL` of `O_(2)` at `STP` will be:

Options

A. 5.4 g
B. 10.8g
C. 54.0 g
D. 108.0 g

Explanation

To find the weight of silver displaced by the quantity of electricity that displaces 5600 mL of O₂ at STP, we can follow these steps:

### Step-by-Step Solution:

1. **Calculate the Moles of O₂:**
At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22400 mL. Therefore, we can calculate the number of moles of O₂ in 5600 mL using the formula:
\[ \text{Moles of O₂} = \frac{\text{Volume of O₂ (mL)}}{22400 \text{ mL/mol}} = \frac{5600}{22400} = \frac{1}{4} \text{ moles} \]

2. **Determine the Moles of Electrons Produced:**
The reaction for the formation of O₂ from oxide involves the transfer of electrons. The balanced reaction can be represented as:
\[ 4 \text{e}^- + 2 \text{H}_2O \rightarrow O_2 + 4 \text{H}^+ \]
This indicates that 1 mole of O₂ requires 4 moles of electrons. Therefore, for \(\frac{1}{4}\) moles of O₂:
\[ \text{Moles of electrons} = \frac{1}{4} \text{ moles O₂} \times 4 \text{ moles e}^- = 1 \text{ mole of electrons} \]

3. **Relate Moles of Electrons to Moles of Silver:**
The reaction for silver can be represented as:
\[ \text{Ag}^+ + \text{e}^- \rightarrow \text{Ag (s)} \]
This shows that 1 mole of Ag is produced by 1 mole of electrons. Thus, 1 mole of electrons will displace 1 mole of silver.

4. **Calculate the Weight of Silver:**
The atomic weight of silver (Ag) is given as 108 g/mol. Therefore, the weight of silver displaced by 1 mole of electrons (which displaces 1 mole of silver) is:
\[ \text{Weight of Ag} = 1 \text{ mole Ag} \times 108 \text{ g/mol} = 108 \text{ g} \]

### Final Answer:
The weight of silver displaced by the quantity of electricity that displaces 5600 mL of O₂ at STP is **108 grams**.

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