the reaction of 6.62g of carbon with excess oxygen yields 13.40g of CO2. what is the percent yield of this reaction

C + O2 ==> CO2

mols C = grams/molar mass
1 mol C forms 1 mol CO2
Then grams CO2 = mols CO2 x molar mass CO2. This is the theoretical yield.
%yield = (actual yield/theo yield)*100 = ?

To calculate the percent yield of a reaction, we need to compare the actual yield with the theoretical yield.

Step 1: Calculate the theoretical yield of CO2.
To determine the theoretical yield, start by determining the molar masses of the substances involved.
The molar mass of carbon (C) is 12.01 g/mol, while the molar mass of carbon dioxide (CO2) is 44.01 g/mol.

Next, calculate the moles of carbon and CO2 using their respective molar masses.
Moles of C = mass of C / molar mass of C
Moles of C = 6.62 g / 12.01 g/mol ≈ 0.55 mol

Since the reaction equation is balanced, we know that 1 mol of carbon reacts to produce 1 mol of CO2.
Therefore, the moles of CO2 produced would be the same as the moles of carbon: 0.55 mol.

Finally, calculate the theoretical yield of CO2.
Theoretical yield of CO2 = moles of CO2 × molar mass of CO2
Theoretical yield of CO2 = 0.55 mol × 44.01 g/mol ≈ 24.21 g

Step 2: Calculate the percent yield.
The percent yield is calculated using the formula:
Percent Yield = (Actual Yield / Theoretical Yield) × 100%

In this case, the actual yield of CO2 is given as 13.40 g, and the theoretical yield is calculated as 24.21 g.

Percent Yield = (13.40 g / 24.21 g) × 100%
Percent Yield = 55.36%

Therefore, the percent yield of this reaction is approximately 55.36%.