[Treetheta]

In a laboratory experiment, 0.03404 g of Mg was completely reacted with dilute, aqueous
HCl generating H₂(g). The H₂(g) was collected in a gas burette over the aqueous solution at
26.4^oC. The final level of aqueous solution in the burette was 5.00 cm higher than the
level in the beaker. The vapour pressure of the aqueous solution at 26.4^oC was 25.8 mm
Hg and the barometric pressure that day was 764.8 mm Hg. Given that the density of the
aqueous solution is 1.00 g/mL and the density of Mg is 13.6 g/mL, calculate the volume
of the H₂(g) that was collected. (atomic mass of Mg = 24.30 g/mol)

I think I am supposed to be using PV = NRT but I'm not sure why they gave the density's or the 5.00 cm higher Its all really confusing me can someone help guide where to start

[Treetheta]

please close this topic i have gotten the answer ty

[kinza]

hey m doign hte same questions i hav gotten the answer but i didnt use the densities at all...did u se the pv=nrt thing??