To find the percent yield of a reaction, we need to compare the actual yield of the product to the theoretical yield, and then express this as a percentage.
First, let's calculate the theoretical yield of carbon dioxide (CO2) using stoichiometry.
From the balanced chemical equation:
2 C2H2 + 5 O2 → 4 CO2 + 2 H2O
We can see that 2 moles of acetylene (C2H2) produce 4 moles of carbon dioxide (CO2).
Molar mass of acetylene (C2H2):
C: 12.01 g/mol
H: 1.01 g/mol
Total: 2(12.01) + 2(1.01) = 26.04 g/mol
Given that we have 2.6 g of acetylene (C2H2), we can calculate the number of moles:
2.6 g / 26.04 g/mol ≈ 0.0998 mol
According to the stoichiometry of the reaction, 0.0998 mol of acetylene (C2H2) will produce:
(4 mol CO2 / 2 mol C2H2) * 0.0998 mol ≈ 0.1996 mol CO2
Now, let's calculate the mass of carbon dioxide (CO2) produced:
Molar mass of carbon dioxide (CO2):
C: 12.01 g/mol
O: 16.00 g/mol
Total: 12.01 + 2(16.00) = 44.01 g/mol
Theoretical yield of CO2:
0.1996 mol * 44.01 g/mol = 8.78 g
Now, let's calculate the percent yield:
Percent yield = (actual yield / theoretical yield) * 100%
= (8.0 g / 8.78 g) * 100%
≈ 91%
Therefore, the percent yield of the reaction is approximately 91%.
