A sample of gas contains 0.1400 mol of C2H4 (g) and 0.1400 mol of Br2 (g) and occupies a volume of 17.3 L. The following reaction takes place: C2H4(g) +Br(g) => CH2BrCH2Br(g)

Calculate the volume of the sample after each reaction takes place, assuming that the temperature and the pressure remain constant.

L

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2