For the balanced equation shown below, how many grams of CO2 would be produced by 48.8 grams of O2? C6H4Cl2 + 7O2 → 6CO2 + 2H2O + Cl2

Answer 1

Calculate Molar Mass(MM):

MM CO₂ = 2x16amu + 12.01amu = 44.01g/mol

MM O₂ = 2x16am = 32g/mol

Calculate amount of CO₂:

48.8gO₂ x molO₂ / 32gO₂ x 6molCO₂ / 7 mol O₂ x 44.01gCO₂ /mol CO₂ = 57.5g CO₂

Answer 2

C₆H₄Cl2 + 7O₂ → 6CO₂ + 2H₂O + Cl₂ 48.8 gm O₂

1. First check if equation is balanced - It is !
2. Whtat is the atomic ass of oxygen - atomic mass of oxygen is 16 gm/mole. Molecular mass of O₂ is 32. So 48.8 gm of O₂ is 48.8gm /(32 gm./mole) = 1.525 moles of O₂.
3. for each 7 moles of O₂ 6 moles of CO₂ are produced, So when 1.525 moles of O2 are consumed, 1.524 (6/7) moles of CO2 are produced That amounts to 1.307 moles of CO₂ is equivalent to 1.307(44) gms of CO2.
4. The molecular mass of CO2 is 12 + 32 = 44 grams.mole. This is equal to 57.5 grams of CO₂.