How much charge is required to produce hydrogen gas at the rate of 1 $mL/s$ by the electrolysis of molten $N a C l$ ?

1.4 C

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18.4 C

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4.3 C

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8.6 C

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Solution

The correct option is D 8.6 C
$1 Equivalent = 11200 ml H_{2} {mol}^{- 1} \equiv 1 {F mol}^{- 1} \equiv 96500 {C mol}^{- 1}$
$Q = n F$
Where, n = number of moles
$Q = \frac{1 ml}{11200 {ml mol}^{- 1}} \times 96500 {C mol}^{- 1} = 8.6 C$

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How much charge is required to produce hydrogen gas at the rate of 1 mL/s by the electrolysis of molten NaCl?

The correct option is D 8.6 C1 Equivalent=11200 ml H2 mol−1≡1 F mol−1≡96500 C mol−1 Q=nF Where, n = number of moles Q=1 ml11200 ml mol−1×96500 C mol−1=8.6 C

How much charge is required to produce hydrogen gas at the rate of 1 $mL/s$ by the electrolysis of molten $N a C l$ ?

The correct option is D 8.6 C
$1 Equivalent = 11200 ml H_{2} {mol}^{- 1} \equiv 1 {F mol}^{- 1} \equiv 96500 {C mol}^{- 1}$
$Q = n F$
Where, n = number of moles
$Q = \frac{1 ml}{11200 {ml mol}^{- 1}} \times 96500 {C mol}^{- 1} = 8.6 C$