a little help with unit 2

[lnaa19]

Hydrogen gas reacts with chlorine gas according to the equation:
H2(g) + Cl2(g) → 2HCl(g)
3.0L of hydrogen and 7.0L of chlorine are allowed to react as much as possible. What will be the volume of the gaseous mixture at the end of the reaction, assuming all volumes are measured at the same temperature and pressure?

I can't get the answer It's 10L btw. Thanks in advance!

[b^3]

c=n/v
v=n/c Since they are proportional we can just use volume here.

So its a 1:1 ratio. So 3L of H₂ reacts with 3L of Cl₂.
So H₂ is the limiting reagent. Amount of Cl₂ left is 7-3=4L
So 2*3=6L of HCl is produced along with the 4L of Cl₂ still remaining.

4+6=10L in total.

[lnaa19]

Thankyou