The gaseous hydrocarbon butane, C4H10, burns according to the following equation: (9.1, 9.2, 9.3, 9.4)
2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(g)
a. How many moles of H2O are produced from the complete reaction of 2.50 mol of C4H10?
b. How many grams of O2 are needed to react completely with 22.5 g of C4H10?
c. How many grams of CO2 are produced from the complete reaction of 55.0 g of C4H10?
d. If the reaction in part c produces 145 g of CO2, what is the percent yield of CO2 for the reaction?
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