How many grams of the adipic acid (C6H10O4) could form from the reaction of 15.00 g of cyclohexane (C6H12) with the 25.00 g of oxygen?
Will the formula be...
2O2 + C6H12 ---> C6H10O4
To determine the amount of adipic acid (C6H10O4) that could form from the given reactants, we can use stoichiometry. The balanced equation you provided is:
2O2 + C6H12 → C6H10O4
First, we need to find the limiting reactant by comparing the amounts of cyclohexane (C6H12) and oxygen (O2). We will use the molar masses of the reactants to convert grams to moles.
The molar mass of cyclohexane (C6H12) is:
(6 carbon atoms x 12.01 g/mol) + (12 hydrogen atoms x 1.01 g/mol) = 84.18 g/mol
The molar mass of oxygen (O2) is:
2 x 16.00 g/mol = 32.00 g/mol
Now, let's calculate the number of moles for each reactant:
Moles of cyclohexane = mass of cyclohexane / molar mass of cyclohexane
Moles of cyclohexane = 15.00 g / 84.18 g/mol ≈ 0.1782 mol
Moles of oxygen = mass of oxygen / molar mass of oxygen
Moles of oxygen = 25.00 g / 32.00 g/mol ≈ 0.7813 mol
Next, we will compare the moles of each reactant to determine the limiting reactant. The limiting reactant is the one that is completely consumed and limits the amount of product that can be formed. In this case, since the stoichiometric ratio between the reactants is 1:2 (2 moles of oxygen for every 1 mole of cyclohexane), we need to convert the moles of cyclohexane to moles of oxygen.
Moles of cyclohexane * (2 moles of oxygen / 1 mole of cyclohexane) ≈ 0.1782 * 2 ≈ 0.3564 mol
Since the moles of oxygen (0.7813 mol) are greater than the calculated moles of cyclohexane (0.3564 mol), the limiting reactant is cyclohexane. Therefore, we will use cyclohexane to determine the maximum possible yield of adipic acid.
Now, we can use stoichiometry to find the number of moles of adipic acid (C6H10O4) produced from the limiting reactant. The stoichiometric ratio between cyclohexane and adipic acid is 1:1.
Moles of adipic acid = moles of cyclohexane = 0.3564 mol
Finally, we can calculate the mass of adipic acid (C6H10O4) formed by multiplying the number of moles by the molar mass of adipic acid.
Mass of adipic acid = moles of adipic acid x molar mass of adipic acid
Mass of adipic acid = 0.3564 mol x [(6 x 12.01 g/mol) + (10 x 1.01 g/mol) + (4 x 16.00 g/mol)]
Mass of adipic acid ≈ 0.3564 mol x 146.15 g/mol ≈ 52.11 g
Therefore, approximately 52.11 grams of adipic acid (C6H10O4) could form from the given reaction.