Determine the mass of the products formed by the combustion of a 7.6g of a coumpound with emprical formula C7H12
C7H12 + 10O2 ==> 7CO2 + 6H2O
moles C7H12 = 7.6g/96 = estimated 0.08
mols CO2 = 0.08mols C7H12 x (7 mols CO2/1 molC7H12) = estimated 0.55
Then mass = mols CO2 x molar mass CO2 = ?
Do the same for mols C7H12 to mols H2O, convert mols H2O to grams. then add the g CO2 + g H2O = total grams products.
To determine the mass of the products formed by the combustion of a compound with the empirical formula C7H12, you need to calculate the molar mass of the compound first. Once you have the molar mass, you can find the mole ratio between the compound and its combustion products to determine the number of moles of each element involved in the reaction.
Step 1: Calculate the molar mass of the compound
To calculate the molar mass of the compound with empirical formula C7H12, determine the molar mass of each element (carbon and hydrogen) and multiply it by the number of atoms in the empirical formula.
Molar mass of carbon (C): 12.01 g/mol
Molar mass of hydrogen (H): 1.01 g/mol
Molar mass of C7H12 = (7 * molar mass of C) + (12 * molar mass of H)
= (7 * 12.01 g/mol) + (12 * 1.01 g/mol)
= 84.07 g/mol + 12.12 g/mol
= 96.19 g/mol
Therefore, the molar mass of the compound is 96.19 g/mol.
Step 2: Determine the combustion products
In the process of combustion, the compound reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). The balanced chemical equation for this reaction is:
C7H12 + 9O2 → 7CO2 + 6H2O
This equation shows that for every 1 mole of C7H12, you get 7 moles of CO2 and 6 moles of H2O.
Step 3: Calculate the mass of the products
To find the mass of the products formed, you need to convert the mass of the compound (given as 7.6 g) to moles using its molar mass. Then, you can use the mole ratio from the balanced chemical equation to determine the moles of CO2 and H2O produced. Finally, convert the moles of each product to grams by multiplying the number of moles by their respective molar mass.
Mass of C7H12 = 7.6 g
Number of moles of C7H12 = Mass / Molar mass
= 7.6 g / 96.19 g/mol
= 0.079 moles
Now, use the mole ratio to determine the moles of CO2 and H2O produced:
Moles of CO2 = 7 moles of CO2 / 1 mole of C7H12 * 0.079 moles of C7H12
= 0.553 moles
Molar mass of CO2 = 44.01 g/mol
Mass of CO2 = Moles * Molar mass
= 0.553 moles * 44.01 g/mol
= 24.32 g
Moles of H2O = 6 moles of H2O / 1 mole of C7H12 * 0.079 moles of C7H12
= 0.474 moles
Molar mass of H2O = 18.02 g/mol
Mass of H2O = Moles * Molar mass
= 0.474 moles * 18.02 g/mol
= 8.54 g
Therefore, the mass of the products formed by the combustion of 7.6 g of the compound with the empirical formula C7H12 is approximately 24.32 g of CO2 and 8.54 g of H2O.