if 5.76 grams of co2 forms when 4.00 grams of c2h6 reacts, what is the percent yield for 2c2h6+7o2=4co2+6h2o
the theoretical yield is 2 moles of CO2 for each mole of C2H6
So,
how many moles of C2H6 did you use?
how many moles of CO2 in 5.76g?
compare your yield with the possible yield.
To find the percent yield of a reaction, you need to compare the actual yield with the theoretical yield. The actual yield is the amount of product that is obtained experimentally, and the theoretical yield is the maximum amount of product that can be obtained based on the stoichiometry of the reaction.
Given:
Mass of C2H6 = 4.00 grams
Mass of CO2 formed = 5.76 grams
First, we need to calculate the theoretical yield of CO2 based on the given mass of C2H6. We can do this by using the stoichiometry of the reaction:
2C2H6 + 7O2 -> 4CO2 + 6H2O
The molar ratio between C2H6 and CO2 is 2:4. Therefore, the moles of C2H6 will be equal to the moles of CO2. To find the moles of C2H6, we can use its molar mass:
Molar mass of C2H6 = 2 * (12.01 g/mol) + 6 * (1.01 g/mol) = 30.07 g/mol
Moles of C2H6 = mass / molar mass = 4.00 g / 30.07 g/mol ≈ 0.133 mol
Since moles of C2H6 and CO2 are equal in this reaction, the theoretical yield of CO2 will also be 0.133 mol.
Now, we need to convert the moles of CO2 to grams using its molar mass:
Molar mass of CO2 = 12.01 g/mol + 2 * (16.00 g/mol) = 44.01 g/mol
The theoretical yield of CO2 is:
Theoretical yield = moles of CO2 * molar mass of CO2 = 0.133 mol * 44.01 g/mol ≈ 5.85 grams
Therefore, the theoretical yield of CO2 is approximately 5.85 grams.
Now we can calculate the percent yield:
Percent yield = (actual yield / theoretical yield) * 100
= (5.76 g / 5.85 g) * 100
≈ 98.5%
The percent yield for the reaction is approximately 98.5%.
To find the percent yield, we need to compare the actual yield with the theoretical yield. The actual yield is the amount of CO2 that was formed, which is given as 5.76 grams. The theoretical yield is the amount of CO2 that would be formed if the reaction went to completion, which can be calculated based on the stoichiometry of the balanced equation.
From the balanced equation:
2C2H6 + 7O2 -> 4CO2 + 6H2O
We can see that the ratio between C2H6 and CO2 is 2:4, which simplifies to 1:2. So for every 2 moles of C2H6, we would expect 4 moles of CO2.
Next, we need to convert the given mass of C2H6 (4.00 grams) to moles using its molar mass. The molar mass of C2H6 is:
2(C) + 6(H) = (2x12.01 g/mol) + (6x1.01 g/mol) = 30.07 g/mol
So, 4.00 grams of C2H6 is equal to:
4.00 g / 30.07 g/mol = 0.133 mol
According to the stoichiometry, the moles of CO2 formed should be twice the moles of C2H6 reacted. Therefore, the theoretical yield of CO2 is:
2 x 0.133 mol = 0.266 mol
Now, we can calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100%:
Percent yield = (Actual yield / Theoretical yield) x 100%
= (5.76 g / (0.266 mol x 44.01 g/mol)) x 100%
≈ 48.6%
So, the percent yield for the reaction 2C2H6 + 7O2 -> 4CO2 + 6H2O is approximately 48.6%.