Question:
What is the total charge of one mole of electrons?
What is the total charge of one mole of electrons?
Show Hint
One mole of electrons carries one Faraday of charge:
\[
1F=96485\ C \approx 9.65\times10^4\ C
\]
This value is frequently used in electrochemistry calculations.
Updated On: Jun 18, 2026
- \(9.65\times10^4\ C\)
- \(9.65\times10^3\ C\)
- \(1.93\times10^5\ C\)
- \(1.602\times10^{-19}\ C\)
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The Correct Option is A
Solution and Explanation
Step 1: Recall the charge on one electron.
The charge on one electron is \[ e=1.602\times10^{-19}\ C \]
Step 2: Recall Avogadro's number.
One mole contains \[ N_A=6.022\times10^{23} \] particles.
Therefore, one mole of electrons contains \[ 6.022\times10^{23} \] electrons.
Step 3: Calculate the total charge of one mole of electrons.
\[ Q=N_A\times e \] \[ Q=(6.022\times10^{23})(1.602\times10^{-19}) \] \[ Q=9.648\times10^4\ C \] \[ Q\approx 9.65\times10^4\ C \] This quantity is known as one Faraday.
Step 4: Final conclusion.
Hence, \[ \boxed{9.65\times10^4\ C} \] Therefore, the correct option is (1).
The charge on one electron is \[ e=1.602\times10^{-19}\ C \]
Step 2: Recall Avogadro's number.
One mole contains \[ N_A=6.022\times10^{23} \] particles.
Therefore, one mole of electrons contains \[ 6.022\times10^{23} \] electrons.
Step 3: Calculate the total charge of one mole of electrons.
\[ Q=N_A\times e \] \[ Q=(6.022\times10^{23})(1.602\times10^{-19}) \] \[ Q=9.648\times10^4\ C \] \[ Q\approx 9.65\times10^4\ C \] This quantity is known as one Faraday.
Step 4: Final conclusion.
Hence, \[ \boxed{9.65\times10^4\ C} \] Therefore, the correct option is (1).
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