Carbon tetrachloride, CCl4 , is a solvent that was once used in large quantities in dry cleaning. Because it is a dense liquid that does not burn, it was also used in fire extinguishers. Unfortunately, its use was discontinued because it was found to be a carcinogen. It was manufactured by the following reaction: CS2 3Cl2 £ CCl4 S2Cl2 The reaction was economical because the byproduct disulfur dichloride, S2Cl2 , could be used by industry in the manufacture of rubber products and other materials. a. What is the percentage yield of CCl4 if 719 kg is produced from the reaction of 410. kg of CS2 . b. If 67.5 g of Cl2 are used in the reaction and 39.5 g of S2Cl2 is produced, what is the percentage yield? c. If the percentage yield of the industrial process is 83.3%, how many kilograms of CS2 should be reacted to obtain 5.00 104 kg of CCl4 ? How many kilograms of S2Cl2 will be produced, assuming the same yield for that product?