If the percent yield for the following reaction is 65.0%, and 30.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq), are produced? 3 NO2(aq) + H2O(l) --> 2 HNO3 (aq) + NO (g)

17.8 grams HNO₃

Explanation:

Given:         3NO₂(g)        + 2H₂O(l) =>          2HNO₃         + NO

             30.0g/46g/mol                           2/3(0.652mol)

             = 0.652mol                                  = 0.435mol (theoretical)

actual yield (65.0%) = 0.65(0.435mol) = 0.283mol(63g/mol) = 17.8 grams HNO₃

um i think it might be a car?