The first step to answering this question is to write out a balanced chemical equation.
3NO2(g) + H2O(l) > 2HNO3(aq) + NO(g)
To assess how much NO2 is needed, we need to know the moles of NO formed. So we convert the grams of NO into the number of moles using the molecular weight of NO (= 30.01 g/mol)
Thus, 180.4 g NO × (1 mol NO/30.01 g NO) = 180.4/30.01 mol NO = 6.011 mol NO
Using the coefficients of the balanced equation we see that for every 3 moles of NO2(g) consumed in the reaction, 1 mol of NO(g) is formed. Thus, mol NO2 = 3 × mol NO = 3 × 6.011 = 18.033 mol NO2
Then, convert the moles of NO2 back into grams using the molecular weight (= 46.006 g/mol)
18.033 mole NO2 × 46.006 g NO2/1 mol NO2 = 18.033 × 46.006 = 829.626 g NO2