Question

Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 128.g of carbon dioxide is produced from the reaction of 83.39 g of octane and 198.6 g of oxygen gas, calculate the percent yield of carbon dioxide.

Be sure your answer has the correct number of significant digits in it.

Answer 1

Solutim We know general equation Catly + (x+Y/4) O2 = 2CO₃ + H2O CH3 (CH2) CH3 Cgtig ..CEthne +(8+18) 2 = 8C0271@ 72 O » Cahid + 25 g = 8 co2 +9h207 128 gm of a produced 83-39 qm Octane = (83 9 mole 20.73 mole - 198.6902 = (148-6) gr more = 12.4 mole. a mole octane Reacts with 12.5 mole O2 Here 0.73 more octane should react with 0.7341218 = 9.05 mol 2 : Limiting Reageat is octane (0.73 more So, (0.73x 8) mole = 9.84 o mole coq should 5.sh mole co2 = (s. 8uxuy) gm = 256.969m 114.23 produce. of yieldita with obtained Yield 'Camscanner Theoretical Yield (Theoretical yield) _x160,- 4918) Soy. CA 95696