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
26.4oC. 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 26.4oC 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