Advertisements
Advertisements
Question
How many electrons flow through a metllic wire if a current of 0·5 A is passed for 2 hours? (Given : 1 F = 96,500 C mol−1)
Advertisements
Solution
I = 0.5 A
t = 2 hours = 2 × 60 × 60 s = 7200 s
Thus, Q = It
= 0.5 A × 7200 s
= 3600 C
We know that 96500 C = 6.023 × 1023 number of electrons.
Then,
3600 C = `(6.023 xx 10^23 xx 3600)/96500` number of electrons
= 2.25 x 1022 number of electrons
Hence 2.25 x 1022 number of electrons will flow through the wire
APPEARS IN
RELATED QUESTIONS
Why cannot we store AgNO3 solution in copper vessel?
Define the following term:
Fuel cell
A solution of CuSO4 is electrolysed using a current of 1.5 amperes for 10 minutes. What mass of Cu is deposited at cathode? [Atomic mass of Cu = 63.7]
How many faradays of electricity are required for the following reaction to occur
\[\ce{MnO^-_4 -> Mn^2+}\]
The electrochemical cell stops working after some time because
If the half-cell reaction A + e– → A– has a large negative reduction potential, it follow that:-
Which of the following is incorrect?
The number of moles of electrons passed when the current of 2 A is passed through a solution of electrolyte for 20 minutes is ______.
What should be the signs (positive/negative) for \[\ce{E^0_{cell}}\] and ΔG0 for a spontaneous redox reaction occurring under standard conditions?
Can we construct an electrochemical cell with two half-cells composed of ZnSO4 solution and zinc electrodes? Explain your answer.
