how many grams of CO2 are produced if 25.0 g of C6H6(BENZENE) was burned?
To determine the number of grams of CO2 produced when 25.0 g of C6H6 (benzene) is burned, we need to use the balanced chemical equation for the combustion of benzene:
C6H6 + 15/2 O2 -> 6 CO2 + 3 H2O
The coefficients in front of each chemical formula represent the ratio of moles. Therefore, we will convert the grams of benzene to moles, then use the stoichiometric coefficients to calculate the number of moles of CO2 produced, and finally convert that to grams of CO2.
1. Find the molar mass of benzene (C6H6):
C: 6 * 12.01 g/mol = 72.06 g/mol
H: 6 * 1.008 g/mol = 6.048 g/mol
Total molar mass = 72.06 g/mol + 6.048 g/mol = 78.108 g/mol
2. Convert grams of benzene to moles:
Moles of benzene = Mass of benzene / Molar mass of benzene
Moles of benzene = 25.0 g / 78.108 g/mol = 0.3202 mol
3. Use the stoichiometric coefficients to determine the moles of CO2 produced:
According to the balanced equation, 1 mole of C6H6 produces 6 moles of CO2.
Moles of CO2 = Moles of benzene * (6 moles CO2 / 1 mole C6H6)
Moles of CO2 = 0.3202 mol * 6 = 1.9212 mol
4. Convert moles of CO2 to grams:
Molar mass of CO2 = 12.01 g/mol (carbon) + 2 * 16.00 g/mol (oxygen) = 44.01 g/mol
Mass of CO2 = Moles of CO2 * Molar mass of CO2
Mass of CO2 = 1.9212 mol * 44.01 g/mol = 84.435 g
Therefore, approximately 84.4 grams of CO2 are produced when 25.0 grams of C6H6 (benzene) is burned.