Question

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)

Answer 1

17.8 grams HNO₃

Step-by-step 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