A sample of gas contains 0.1800 mol of and 0.09000 mol of and occupies a volume of 11.9 L. The following reaction takes place:2HCI(g) +Br_2(g) --->2HBr(g) +Cl_2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = ___ L

A sample of gas contains 0.1700 mol of CH4(g) and 0.1700 mol of H2O(g) and occupies a volume of 19.2 L. The following reaction takes place:CH4(g) + H2O(g)3H2(g) + CO(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

A sample of gas contains 0.150 mol of N₂(g) and 0.300 mol of H₂(g) and occupies a volume of 21.4 L. The following reaction takes place: N₂(g) + 2H₂(g)-N₂H4(9) Calculate the volume of the sample after the reaction takes place (assume temperature and pressure are constant).

Vol 752mL Gas X  (g) 2.49g 1.98 atm 62oC     Identity of the gas - by formula ?

The reaction shown below occurs in a sealed container: 2 NH3 (g) --> N2 (g) + 3 H2 (g) What is true about the gases in the container as the reaction proceeds? None of these answers is correct. OThe mass remains constant, and the number of molecules increases The mass remains constant, and the pumber of molecules decreases O The mass increases, and the number of molecules increases The mass decreases, and the number of molecules increases