Question

# Carbon disulfide (CS2) reacts with excess chlorine (Cl2) to produce carbon tetrachloride (CCl4) and disulfur dichloride...

Carbon disulfide (CS2) reacts with excess chlorine (Cl2) to produce carbon tetrachloride (CCl4) and disulfur dichloride (S2Cl2). If 53.2 g of CS2 yields 84.2 g of CCl4, what is the percent yield? (Hint, you must first write the balanced equation.)

Molar mass of CS2,
MM = 1*MM(C) + 2*MM(S)
= 1*12.01 + 2*32.07
= 76.15 g/mol

mass(CS2)= 53.2 g

number of mol of CS2,
n = mass of CS2/molar mass of CS2
=(53.2 g)/(76.15 g/mol)
= 0.6986 mol
Balanced chemical equation is:
CS2 + 4 Cl2 ---> CCl4 + 2 S2Cl2

Molar mass of CCl4,
MM = 1*MM(C) + 4*MM(Cl)
= 1*12.01 + 4*35.45
= 153.81 g/mol

According to balanced equation
mol of CCl4 formed = (1/1)* moles of CS2
= (1/1)*0.698621
= 0.698621 mol

mass of CCl4 = number of mol * molar mass
= 0.6986*1.538*10^2
= 1.075*10^2 g

% yield = actual mass*100/theoretical mass
= 84.2*100/107.454918
= 78.4 %

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