Propane (C3H8) burns in oxygen to produce carbon dioxide and water via the following reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)...
Propane (C3H8) burns in oxygen to produce carbon dioxide and water via the following reaction:
C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)
Calculate the mass of CO2 that can be produced if the reaction of 49.9 g of propane and sufficient oxygen has a 60.0 % yield.
Homework Answers
Balanced chemical equation is:
C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)
No. of moles of propane = (49.9 g) / (44.10 g/mol) = 1.13 mol
No. of moles of CO2 produced = (3 / 1) x 1.13 mol = 3.39 mol
Theoretical yield of CO2 = (3.39 mol) x (44.01 g/mol) = 149.4 grams
Given; yield of the reaction is 60.0 %
Mass of CO2 produced = (149.4 g) x (60 %) = 89.64 grams of CO2 formed in this reaction
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