Phosgene (98.92 g/mol)can be formed from carbon monoxide (28.01 g/mol)and chlorine gas (70.90 g/mol)according to the following reaction: CO(g)+ Cl₂(g)$\to$ COCl₂(g) How many grams of COCl₂ can be produced when 0.772 atm CO and 0.753 atm Cl₂ are mixed in a 260 L tank at 323 K,assuming 100% yield?

Question

Quizplus · Accepted Answer

The balanced chemical equation is:CO(g) + Cl2(g) → COCl2(g)The mole fraction of CO is:XCO = PCO / (PCO + PCl2) = 0.772 atm / (0.772 atm + 0.753 atm) = 0.507The mole fraction of Cl2 is:XCl2 = PCl2 / (PCO + PCl2) = 0.753 atm / (0.772 atm + 0.753 atm) = 0.493The total number of moles of gas in the tank is:n = (P * V) / (R * T) = (1.525 atm * 260 L) / (0.0821 L atm / mol K * 323 K) = 12.5 molThe number of moles of COCl2 produced is:nCOCl2 = XCO * n = 0.507 * 12.5 mol = 6.34 molThe mass of COCl2 produced is:mCOCl2 = nCOCl2 * MW = 6.34 mol * 98.92 g/mol = 626 gTherefore, the correct answer is A: 760 g.

Phosgene (98 →\to→ COCl2(g) How Many Grams of COCl2 Can Be Produced When

Phosgene (98 $\to$ COCl₂(g)
How Many Grams of COCl₂ Can Be Produced When