A mixture of 58.0 of S and 1.01 Solution First write the chemical reactions (bal

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First write the chemical reactions (balanced): S + Cl2 -> SCl2 2S + Cl2 -> S2Cl2 Calculate the moles of each reactant atom: moles S = (50g)/(32g/mole) = 1.563 moles S moles Cl = (100g)/(35.453g/mole) = 2.820 moles Cl let x = moles SCl2 let y = moles S2Cl2 then: x + 2y = 1.563 (mass balance on moles of S) 2x + 2y = 2.820 (mass balance on moles of Cl) Solve for x and y: => rearrange 2nd equation: 2y = 2.820 - 2x => substitute into 1st equation: x + (2.820-2x) = 1.563 => simplify: 2.820 -x = 1.563 => solve for x : x= 2.820 - 1.563 = 1.257 moles SCl2 Solve for y from 1st equation: x + 2y = 1.563 => 2y = 1.563 -x => y= (1.563-x)/2 = (1.563 - 1.257)/2 = 0.153 moles S2Cl2

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