Methane (CH4, 16.05 g/mol) reacts with oxygen to form carbon dioxide (CO2, 44.01 g/mol) and water (H2O, 18.02 g/mol). Assume that you design a system for converting methane to carbon dioxide and water. To test the efficiency of the system in the laboratory, you burn 5.00 g methane. The actual yield is 6.10 g water. What is your percent yield?
Answers
Answer:
The percent yield of reaction is 54.32%.
Explanation:
Moles of methane =
According to reaction, 1 mole of methane gives 2 moles of water .
The 0.3115 moles of methane will give:
of water
Mass of 0.9345 moles of water = 0.623 mol × 18.02 g/mol = 11.23 g.
Theoretical yield of methane = 11.23 g.
Experimental yield of methane = 6.10 g.
The percent yield of reaction:
The percent yield of reaction is :
Answer:54.5
Explanation:
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liquid
solid and gas
liquid and solid
Answers
Answer:
Liquid
Explanation:
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Answer:
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A.) 6.8 mol
B.) 13.7 mol
C.) 54.8 mol
D.) 109.6 mol
Answers
2 mol H2 ----------- 1 mol O2
27.4 mol H2- ------ x mol O2
2x = 27.4
x = 27.4 / 2
x = 13.7 moles O2
answer b
hope this helps!.
Answer:
B.) 13.7 mol
Explanation:
Edge 2020
b. research
c. intuition
Answers
b. research
c. intuition
Without research you can not conclude if your statement or facts are right.
B. atomic number.
C. molecular mass.
D. molecular size.
Answers