Question

You have 2.2 mol Xe and 2.2 mol F2, but when you carry out the reaction you 0.25 mol XeFa. What is the percent yield of this experiment? Xe(g) +2 F2 (g)XeFa (g) with only dn end

Answer 1

Balanced chemical equation is:

Xe + 2 F2 ---> XeF4 +

1 mol of Xe reacts with 2 mol of F2

for 2.2 mol of Xe, 4.4 mol of F2 is required

But we have 2.2 mol of F2

so, F2 is limiting reagent

we will use F2 in further calculation

According to balanced equation

mol of XeF4 formed = (1/2)* moles of F2

= (1/2)*2.2

= 1.1 mol

% yield = actual mol * 100 / theoretical mol

= 0.25 * 100 / 1.1

= 23 %

Answer: 23 %