Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of carbon dioxide formed from the reaction of 1.80g of ethane and 11.4g of oxygen gas? Round your answer to 3 significant figures.
• Firstly balanced the chemical equation
2C2H6 + 7O2 ------> 4CO2 + 6H2O
• calculate no. Of moles of reactant.
Molar mass of ethane = 30.07g/mol and CO2 = 44.01g/mol and mass of O2 = 32g/mol
a) no. Of moles of C2H6 = 1.80/(30.07) = 0.05986mol
b) no. Of moles of O2 = 11.4/( 32 ) = 0.35625mol
From the above Reaction; theoretical yield always calculate by the limiting reagent. Here limiting reagent is C2H6 because it is totally consumed in the reaction( because it's contains less no. Of moles than oxygen)
2mole of C2H6 produces = 4moles of CO2
0.05986mol of C2H6 produces = 0.05986 • ( 4/2) moles of CO2
No. Of moles of CO2 = 0.05986 • ( 4/2) = 0.11972moles.
Mass of CO2 produces = 0.11972 • 44.01 = 5.2689g
Answer,
Theoretical yield of CO2 = 5.27g ( in 3 signing figure)
Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and...
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