Question

During electrolysis of molten sodium chloride the time required

Answer 1

Answer:The time required to produce 0.10 mol of chlorine gas using a current of 3 ampere is 6433.3 seconds.

Explanation: Q=I\times t

where Q= quantity of electricity in coloumbs

I = current in amperes = 3 A

t= time in seconds = ?

NaCl\rightarrow Na^++Cl^-

2Cl^{-}\rightarrow Cl_2+2e^{-1}

1 mole of electrons carry charge= 96500 C.

96500\times 2=193000Coloumb of electricity deposits 1 mole of Cl_2

1 mole of Cl_2 is deposited by 193000 C

Thus 0.10 moles of Cl_2 is deposited by=\frac{193000}{1}\times 0.10=19300C

19300C=3A\times t

t=6433.3 sec

Answer 2

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$\huge{\mathfrak\red{Here \:is \:your \:answer}}$

$\huge{\mathcal\pink{Question}}$

During electrolysis of molten sodium chloride the time required?

$\huge{\mathcal\pink{Answer:-}}$

The time required to produce 0.10 mol of chlorine gas using a current of 3 ampere is 6433.3 seconds.

Explanation:

Q = I \ times t

where Q= quantity of electricity in colombs.

I = Current of amperes = 3 A

T = Time in seconds = ?

NaCI \ Rightnaarow Na^++CI^-

2CI^{-}\rightarrow CI_2 + 2e^{-1}

1 mole of electrons charge= 96500 C

96500 \ times 2 = 193000 Columb of electricity deposit 1mole of CI_2

1 mole of CI_2 is deposited by 193000 C

Thus, 0.10 mole of CI_2 is deposited by= $\frac{193000}{1}time$

0.10 = 19300 C

19300 C = 3A \ time T

T = 6433.3 seconds

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