Stoichiometry?

Question

Nitrogen dioxide from exhoust reacts with oxygen to form ozone. What mass of ozone could be formed from 4.55 g NO2? If only 4.58 g O3formed, what is the percentage yield?

NO2(g) + O2(g) ----> NO(g) + O3(g)

Answer 1

4.55 g of NO2 is 4.55g/(14+32 g/mol) = 0.0989

Mole to mole ratio from the equation is 1 to 1 between NO2 and 03 since the constants are 1 in front of ea of those terms.

now convert this number of moles into grams.

0.0989moles * (3*16 g/mol) = 4.75grams.

you are told that the actual yield is 4.58.

%yield = 4.58/4.75 * 100% ~ 96%