anonymous
  • anonymous
Fan and medal!!!! Carbon disulfide burns with oxygen to form carbon dioxide and sulfur dioxide in the following manner: CS2 + 3O2 CO2 + 2SO2 If 114 grams of CS2 are burned in an excess of O2 (an amount sufficient to completely burn all 114 g of CS2), how many moles of SO2 are formed? (Remember to follow significant figure rules).
Chemistry
  • Stacey Warren - Expert brainly.com
Hey! We 've verified this expert answer for you, click below to unlock the details :)
SOLVED
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.
schrodinger
  • schrodinger
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
anonymous
  • anonymous
moles CS2 = 114 g/76.143 g/mol= 1.50 the ratio between CS2 and SO2 is 1 : 2 moles SO2 formed = 1.50 x 2 = 3.00

Looking for something else?

Not the answer you are looking for? Search for more explanations.