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secure https://session.masteringchemistry.com/myct/itemView?assignmenProblemD-S004657 Chapter 09 Homework Problem 9.76 Part C How many grams of CO2 are produced from the complete reaction of 52.5 g of CH1o? Express your answer with the appropriate units m(CO2) Value Units Submit My Answers Give Up Part D If the reaction in part e produces 133 g of CO2. what is the percent yield of CO2 for the reaction? Express your answer with the appropriate units. The percent yield ofCO2 Value Units Submit My Answers Give UpExplanation / Answer
C)
Molar mass of C4H10 = 4*MM(C) + 10*MM(H)
= 4*12.01 + 10*1.008
= 58.12 g/mol
mass of C4H10 = 52.5 g
mol of C4H10 = (mass)/(molar mass)
= 52.5/58.12
= 0.9033 mol
we have the Balanced chemical equation as:
2 C4H10 + 13 O2 ---> 8 CO2 + 10 H2O
From balanced chemical reaction, we see that
when 2 mol of C4H10 reacts, 8 mol of CO2 is formed
mol of CO2 formed = (8/2)* moles of C4H10
= (8/2)*0.9033
= 3.6132 mol
Molar mass of CO2 = 1*MM(C) + 2*MM(O)
= 1*12.01 + 2*16.0
= 44.01 g/mol
mass of CO2 = number of mol * molar mass
= 3.6132*44.01
= 159 g
Answer: 159 g
D)
% yield = actual mass*100/theoretical mass
= 133*100/159
= 83.6 %
Answer: 83.6 %
Feel free to comment below if you have any doubts or if this answer do not work. I will edit it if you let me know
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