The balanced equation tells us that 2 moles of propene react with 9 moles of oxygen gas to produce 6 moles of carbon dioxide.
From the given mass of propene (100 g), we can determine the number of moles using its molar mass:
100 g / 42 g/mol = 2.38 mol
Since 2 moles of propene should produce 6 moles of carbon dioxide (according to the balanced equation), we can calculate the theoretical yield of carbon dioxide:
2.38 mol C3H6 x (6 mol CO2 / 2 mol C3H6) x (44 g CO2 / 1 mol CO2) = 251.52 g CO2
Therefore, the percent yield of carbon dioxide is:
(Actual yield / Theoretical yield) x 100%
= (200 g / 251.52 g) x 100%
= 79.4%
Propene, C3H6 (100 g) was subjected to combustion. The actual yield of carbon dioxide is 200 g. Calculate the percent yield of carbon dioxide.
2 C3H6 + 9 O2 → 6 H2O+ 6 CO2
(Molar mass: C=12 g/mol; H= 1g/mol; O =16 g/mol)
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