Question

$0.4\, g$ of dihydrogen is made to react with $7.1 \,g$ of dichlorine to form hydrogen chloride. The volume of hydrogen formed at $273\,K$ and $1$ bar pressure is

• A. 9.08L
• B. 4.54L
• C. 90.8L
• D. 45.4L

Answer 1

Answer: (B)

4.54L

Answer 2

The corresponding balanced reaction is:

$H _{2}+ Cl _{2} \rightarrow 2 HCl$

Again, $0.4 \,g H _{2}=0.4 / 2 \,mol =0.2 \,mol$
$7.1 \, g Cl _{2}=7.1 / 71 \,mol =0.1 \,mol$

So, $Cl _{2}$ is the limiting reagent here.

Hence $0.2$ moles of $HCl$ will be formed.

Again, we need to find out the volume of $HCl$ formed in the STP condition.

1 mol of gas in STP occupies $22.7 \, L$

Thus, $0.2$ mol of $HCl$ will occupy $=4.54 \, L$