An herbicide contains only c, h, cl, and n. the complete combustion of a 200.0 mg sample of the herbicide in excess oxygen produced 209.2 ml of co2 and 122.0 ml of h2o vapor at stp. a separate analysis determined the 200.0 mg sample contained 55.14 mg cl. determine the percent composition of the herbicide.

%C = 56,1%

%H = 5,5%

%Cl = 27,6%

%N = 10,8%

Explanation:

The moles of CO₂ are the same than moles of C in the herbicide.

Moles of H₂O are ¹/₂ of moles of H in the herbicide.

Moles of CO₂ are obtained using:

n = PV/RT

Where, in STP: P is 1 atm; V is 0,2092L; R is 0,082atmL/molK; T is 273 K

moles of CO₂ are: 9,345x10⁻³ mol≡ mol of C×12,01g/mol = 0,1122 g of C ≡ 112,2mg of C

In the same way, moles of H₂O are 5,450x10⁻³mol×2 =0,1090 mol of H×1,01g/mol = 0,0110 g of H ≡ 11,0mg of H

As you have 55,14 mg of Cl, the mg of N are:

200,0mg - 112,2 mg of C - 11,0 mg of H - 55,14 mg of Cl = 21,66 mg of N

Thus, precent composition of the herbicide is:

%C = ×100 = 56,1%C

%H = ×100 = 5,5%H

%Cl = ×100 = 27,6%Cl

%N = ×100 = 10,8%N

I hope it helps!

idk what the question is about