Question

how many faradays of electricity are required to produce 6 g of Mg from MgCl2​

Answer 1

Answer:

0.25 F is required

Explanation:

To ionise one mole any substance 1 F of electricity is required

and 1 mole of MgCl2 contains 24 g of Mg

But only 6 g is required

therefore ., 1/4 F is required

Answer 2

Answer: The number of faradays of electricity required by given amount of magnesium is 0.493 F.

Explanation:

In the given compound of $MgCl_2$, magnesium is present in +2 oxidation state.

To form a neutral atom of magnesium, it requires 2 electrons.

$Mg^{2+}+2e^-\rightarrow Mg$

1 mole of magnesium requires 2 electrons. So, charge on 2 electrons will be 2F.

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

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of magnesium = 6 g

Molar mass of magnesium = 24.31 g/mol

Putting values in above equation, we get:  

$\text{Moles of magnesium}=\frac{6g}{24.31g/mol}=0.246mol$

Using unitary method, we get:

As, 1 mole of magnesium requires a charge of 2 faradays.

So, 0.264 moles of magnesium will require a charge of = $\frac{2}{1}\times 0.264=0.493F$

Hence, the number of faradays of electricity required by given amount of magnesium is 0.493 F.