The amount of charge carried by 1 mole of electrons is the same as carried by a `K^(o+)` ion. True/False

Explanation

To determine whether the statement "The amount of charge carried by 1 mole of electrons is the same as carried by a \( K^{+} \) ion" is true or false, we can follow these steps:

### Step 1: Understand the charge of one mole of electrons
1. The charge of a single electron is approximately \( 1.602 \times 10^{-19} \) coulombs.
2. To find the charge carried by one mole of electrons, we use Avogadro's number, which is \( 6.022 \times 10^{23} \) particles/mole.
3. Therefore, the total charge \( Q \) carried by one mole of electrons is calculated as:
\[ Q = (1.602 \times 10^{-19} \, \text{C}) \times (6.022 \times 10^{23} \, \text{mol}^{-1}) = 96500 \, \text{C} \]
This value is known as one Faraday.

### Step 2: Understand the charge of \( K^{+} \) ion
1. The potassium ion \( K^{+} \) has a single positive charge.
2. The charge carried by one mole of \( K^{+} \) ions is also equal to one Faraday, which is \( 96500 \, \text{C} \).

### Step 3: Compare the charges
1. Since both one mole of electrons and one mole of \( K^{+} \) ions carry the same amount of charge, which is \( 96500 \, \text{C} \), we can conclude that the statement is true.

### Conclusion
The statement "The amount of charge carried by 1 mole of electrons is the same as carried by a \( K^{+} \) ion" is **True**.

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