The number of electrons delivered at the cathode during electrolysis by a current of $1$ ampere in $60$ seconds is (change on electron = $1.60 \times 10^{-19} C)$
- $6 \times 10^{23}$
- $6 \times 10^{20}$
- $3.75 \times 10^{20}$
- $7.48 \times 10^{23}$
The Correct Option is C
Solution and Explanation
Charge and Number of Electrons Calculation
The relationship between charge (\( Q \)) and the number of electrons (\( n \)) is given by:
\(Q = ne\)
The total charge is also related to current and time:
\(I \times t = ne\)
To find the number of electrons, we can solve for \( n \):
\(n = \frac{I \times t}{e}\)
Substituting the given values (current = 1 A, time = 60 seconds, and the elementary charge \( e = 1.6 \times 10^{-19} \) C):
\(n = \frac{1 \times 60}{1.6 \times 10^{-19}}\)
Finally, calculating \( n \):
\(n = 3.75 \times 10^{20}\)
Conclusion:
The number of electrons is \( 3.75 \times 10^{20} \).
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Concepts Used:
Electrolysis
Electrolysis:
Electrolysis is the process by which an element is decomposed and undergoes some chemical change under the influence of any electric current. The first-ever electrolysis was executed out by Sir Humphrey Davey in the year 1808. Electrolysis can occur in both Galvanic cells and Electrolytic cells.
Applications of Electrolysis:
- Electrolytic cells are used for the production of Hydrogen and Oxygen gas from water.
- They are used for the large-scale production of pure metals like sodium, copper, magnesium, etc.
- They are used to extract Aluminium from Bauxite.
- Electrolytic cells are used for electroplating, a process by which a thin protective layer of one metal is formed over another metal, mostly for protection.
- Electrolysis is used for the electrorefining of non-ferrous metals.
Read More: Products of Electrolysis