Given this equation: CH4 + 2O2 = CO2 + 2H2O a)If the percent yield for this reac

Question

Given this equation: CH4 + 2O2 = CO2 + 2H2O a)If the percent yield for this reaction is 95.0%, what actual yield can you expect? b) How many grams of the excess reaction (if there is one) will remain unreacted? 1mol CH4 reacts with 2mol O2 to produce 1mol CO2 and 2mol H2O You have 2.55mol CH4, which will require 2.55*2 = 5.1mol O2. You have only 4.5mol O2, so this is limiting. Concentrate only on the O2 - forget the CH4 When reacting with excess CH4: 2mol O2 produce 1 mol CO2 and 2mol H2O 4.5 mol O2 will produce 4.5/2 = 2.25mol CO2 and 4.5mol H2O Molar mass CO2 = 12.011+15.999*2 = 44.009g/mol 2.25mol = 44.009*2.25 = 99.02g CO2 produced Molar mass H2O = 1.008*2 + 15.999 = 15.015g/mol 4.5mol = 4.5*18.015 = 81.07g H2O produced.

Explanation / Answer

CO2

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