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Methanol (CH4O), which is used as a fuel in high-performance racing cars, burns in the presence of O2 to form CO2 and H2O. The molar masses for all substances are given under the balanced equation.
2CH4O (l) + 3O 2 (g) → 2CO 2 (g) + 4H 2O(g)
32.04 g/mol 32.00 g/mol 44.01 g/mol 18.02 g/mol
a. What is the theoretical yield of CO 2 from 35.0 g of methanol?
b. What is the percent yield of CO 2 if 26.8 g of CO 2 are formed?
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Based on our data, we think this problem is relevant for Professor Randles' class at UCF.