Question

Current required to displace 1g of H2 in 10sec .will be

Answer 1

n=m/M=1g/2=0,5 moles

N=n x L = m/M x L= 0,5 x 6.022×10^23=3.011×10^23

1g of H2 contains 3.011×10^23 atoms

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Answer 2

9650 Ampere is required to displace 1g of $H_2$ in 10 sec

Explanation:

According to mole concept:

1 mole of an atom contains $6.022\times 10^{23}$ number of particles.

We know that:

Charge on 1 electron = $1.6\times 10^{-19}C$

Also, copper will produce 2 electrons. So, out of 5 moles of copper, 10 moles of electrons will be produced.  

So,  

Charge on 10 mole of electrons = $10\times 1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{1g}{2g/mol}=0.5mol$

$2H^++2e^-\rightarrow H_2$

1 mole of hydrogen is displaced by=  $2\times 96500C=193000C$

0.5 mole of hydrogen is displaced by=  $\frac{193000C}{1}\times 0.5=96500C$

To calculate the current required, we use the equation:

$I=\frac{q}{t}$

where,

I = current passed = ?

q = total charge = 96500 C

t = time required = 10 sec

Putting values in above equation, we get:

$I=\frac{96500C}{10s}=9650A$

Hence, the current required is 9650 A

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