Question

23. An important intermediate reaction in the industrial production process of nitric acid is shown. What is the theoretical yield of H2O (18.02 g/mol) if 45.0 kg of NH3 (17.04 g/mol) reacts with excess O2 (32.00 g/mol)? NH3(g) + O2(g) → NO(g) + H2O (1) 24. A 10.00 g sample of a hydrocarbon (which is a compound that contains only carbon and hydrogen) was burned in oxygen, and the carbon dioxide and water produced were carefully collected and weighed. The mass of the carbon dioxide was 34.34 g, and the mass of the water was 5.62 g. What was the empirical formula of the hydrocarbon?

Answer 1

(23) Given reaction NH (9) + 02 (9) NO(g) + +90(e) from the above equation, this is not balanced. Balanced equation is 2N44(34 28 (9) — 2N019) + 34 014) : 2 moles of Ny produce 3 moles of the 2x17:04g of NH3 3x (18.02g) of the 34.089 of NH3 54.069 of tho 45 kg of Nis is used & 45x10²g of Nys t: 1kg = 1000g = 10²9) .: 54.069 of the 34:089 of NH x(45x10°g of way ) = 71.38x1039 of 10 Theoretical yield of tho = 71.38X1039 =71.38 kg =71.4kg