Question

Calculate the volume of $C{l}_2$ at NTP produced during electrolysis of $MgC{l}_2$ which produces $6.50gMg$.
(At. mass of $Mg=24.3)$.

• A. $6litre$.
• B. $6.99litre$.
• C. $4.99litre$.
• D. $3.99litre$.

Answer 1

The correct option is A $6litre$.

From the formula of magnesium chloride $\left(MgC{l}_2\right)$:

One mole of $MgC{l}_2$ gives 1 mole of Mg (24g) and one mole of Chlorine gas $\left(C{l}_2\right)$

One mole of gas occupies 22.4 liters (22400 cm³) at S.T.P.

⇒ 24g of Mg ≡ 22400 cm³ of Chlorine gas at S.T.P.

∴ 6.5 g of Mg ≡ (22400 x 6.5) ÷ 24

≡ 6066.67 cm³ = 6 litre