C2H6(g) + O2(g) CO2(g) + H2O(g)

(a) Consider the unbalanced equation above. What is the maximum mass of CO2 that can be produced when 21.0 g of C2H6 and 38.5 g O2 react?

(b) If 24.7 g of carbon dioxide is actually produced by the reaction in part (a), what is the percent yield for this reaction?

Another LR problem. Follow that last problem I did for you to calculate mass CO2. This is the theoretical yield.

b. For % yield = (actual yield/theor yield)*100 = ?

To solve these problems, we need to go through the steps of balancing the chemical equation and then using stoichiometry to find the desired values.

(a) Balancing the equation:
To balance the chemical equation, we need to make sure that the number of atoms of each element is equal on both sides of the equation.

C2H6(g) + O2(g) -> CO2(g) + H2O(g)

The balanced equation is:

2C2H6(g) + 7O2(g) -> 4CO2(g) + 6H2O(g)

Now we can use stoichiometry to find the maximum mass of CO2 produced.

Step 1: Calculate the number of moles of C2H6 and O2:
The molar mass of C2H6 (ethane) is 30.07 g/mol.
The molar mass of O2 (oxygen gas) is 32.00 g/mol.

Number of moles of C2H6 = mass / molar mass = 21.0 g / 30.07 g/mol = 0.698 mol
Number of moles of O2 = mass / molar mass = 38.5 g / 32.00 g/mol = 1.203 mol

Step 2: Apply stoichiometry to find the moles of CO2 produced:
From the balanced equation, we know that 2 moles of C2H6 react to produce 4 moles of CO2, so the mole ratio is 2:4, or 1:2.
Therefore, the number of moles of CO2 produced = (0.698 mol C2H6) x (2 mol CO2 / 2 mol C2H6) = 0.698 mol.

Step 3: Calculate the mass of CO2 produced:
The molar mass of CO2 (carbon dioxide) is 44.01 g/mol.

Mass of CO2 produced = number of moles x molar mass = 0.698 mol x 44.01 g/mol = 30.69 g.
Therefore, the maximum mass of CO2 that can be produced is 30.69 g when 21.0 g of C2H6 and 38.5 g of O2 react.

(b) To calculate the percent yield, we need to compare the actual yield to the theoretical yield.

Given: Actual yield of CO2 = 24.7 g.

Step 1: Calculate the theoretical yield of CO2 using the balanced equation:
From part (a), we found that the theoretical yield of CO2 is 30.69 g.

Step 2: Calculate the percent yield:
Percent yield = (Actual yield / Theoretical yield) x 100
Percent yield = (24.7 g / 30.69 g) x 100 = 80.5%

Therefore, the percent yield for this reaction is 80.5%.