Acetylene gas, c2h2, burns in oxygen to produce carbon dioxide and water. If 61.4 g of co2 are produced when 22.7g c2h2 react with sufficient oxygen, what is the percent yield for the reaction?
To find the percent yield for the reaction, we need to compare the actual yield (the amount of CO2 produced) to the theoretical yield (the maximum amount of CO2 that can be produced).
First, let's calculate the theoretical yield of CO2. We can use the balanced chemical equation to determine the stoichiometry of the reaction:
C2H2 + O2 → CO2 + H2O
From the equation, we can see that the ratio of C2H2 to CO2 is 1:1. This means that for every 1 mole of C2H2 reacted, 1 mole of CO2 will be produced.
To calculate the moles of CO2 produced, we need to convert the given mass of C2H2 and CO2 to moles using their molar masses.
The molar mass of C2H2 is:
2(C) + 2(H) = 2(12.01 g/mol) + 2(1.01 g/mol) = 26.04 g/mol
The molar mass of CO2 is:
1(C) + 2(O) = 1(12.01 g/mol) + 2(16.00 g/mol) = 44.01 g/mol
Let's calculate the moles of C2H2:
22.7 g C2H2 * (1 mol C2H2 / 26.04 g C2H2) = 0.871 mol C2H2
Since the ratio of C2H2 to CO2 is 1:1, the moles of CO2 produced will also be 0.871 mol.
Now let's calculate the actual yield of CO2, which is given as 61.4 g.
The percent yield is calculated using the formula:
Percent Yield = (Actual Yield / Theoretical Yield) * 100%
Substituting the values:
Percent Yield = (61.4 g CO2 / 0.871 mol CO2) * 100% = 70.55%
Therefore, the percent yield for the reaction is approximately 70.55%.
To find the percent yield for the reaction, we need to compare the actual yield (61.4 g CO2) to the theoretical yield.
To calculate the theoretical yield of CO2, we need to use the balanced equation for the reaction:
C2H2 + 2.5 O2 -> 2 CO2 + H2O
From the equation, we can see that 1 mole of C2H2 reacts with 2 moles of CO2. So, we need to convert the given mass of C2H2 to moles:
Molar mass of C2H2 = 2(12.01 g/mol) + 2(1.01 g/mol) = 26.04 g/mol
Moles of C2H2 = (mass of C2H2) / (molar mass of C2H2) = 22.7 g / 26.04 g/mol = 0.871 mol
Since 1 mol of C2H2 produces 2 mol of CO2, the theoretical yield of CO2 is:
Theoretical yield of CO2 = (moles of C2H2) x (2 mol CO2 / 1 mol C2H2) = 0.871 mol x 2 = 1.742 mol
Now, we can calculate the percent yield:
Percent yield = (Actual yield / Theoretical yield) x 100
Percent yield = (61.4 g / (1.742 mol x molar mass of CO2)) x 100
Molar mass of CO2 = 12.01 g/mol + 2(16.00 g/mol) = 44.01 g/mol
Percent yield = (61.4 g / (1.742 mol x 44.01 g/mol)) x 100
Percent yield ≈ 79.9%
Therefore, the percent yield for the reaction is approximately 79.9%.
Here is an example. Just follow the steps. Using these steps, solve for the theoretical yield, then follow the percent yield part of the example.
http://www.jiskha.com/science/chemistry/stoichiometry.html