One mole of oxygen equal to how much gram equivalent
Answers
“When calculating the molar mass of a compound, are you calculating the molar mass of one mole of the compound?” You are calculating the mass of one mole of the compound. To say “the molar mass of one mole” is not merely redundant, but pointless: molar mass is an intensive property (independent of quantitity) not an extensivive property (depends on quantity). It would be like saying “the formula of one gram of water”; the formula does not depend on the amount.
“If so, can someone explain how adding the molar masses of constituent elements (example CO2) would equal to 1 mole of CO2?” Well, the mass of a molecule is just the sum of the masses of its component atoms (disregarding the mass-equivalent of the energy released when the molecule forms, because it’s too small to measure). For instance, if you had a dozen CO₂ molecules, they would comprise a dozen carbon atoms and two dozen oxygen atoms, so they’d weigh as much as a dozen carbon atoms and two dozen oxygen atoms. This is true even if we replace “dozen” with a much larger number. If you had 600 billion trillion CO₂ molecules, you’d have 600 billion trillion carbon atoms and 1200 billion trillion oxygen atoms. Which is to say, if you have a mole of CO₂ molecules, you’ve got a mole of carbon atoms and two moles of oxygen atoms. So the mass of a mole of CO₂ is the mass of a mole of carbon atoms plus the mass of two moles of oxygen atoms.