Percentage yield calculations

A chemist treated 22.99 g of galantamine with sulfuric acid to make the sulfate salt: $\ce{2C17H21NO3 + H2SO4 -> (C17H22NO3)2SO4}$ The mass of salt isolated was 24.65 g. Determine the percentage yield of the salt. Use section 7 of the data booklet.

(i) If the reaction has a percentage yield of 80 %, calculate the mass, in g, of benzene that would be produced from 2.0 kg of cyclohexane. (ii) Calculate the atom economy for this reaction, as a percentage.

Nitrogen gas is reacted with excess hydrogen gas to produce ammonia. $\ce{N2(g) + 3H2(g) -> 2NH3(g)}$ The reaction of 28.0 g of $\ce{N2}$ with excess $\ce{H2}$ produces 25.5 g of $\ce{NH3}$. What is the percentage yield of $\ce{NH3}$? A. 25% B. 50% C. 75% D.…

Ammonia is oxidized according to the equation below. $\ce{4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g)}$ What is the amount, in mol, of $\ce{H2O}$ produced when 8.00 mol of $\ce{NH3}$ reacts with 5.00 mol of $\ce{O2}$, if the yield is 80 %? A. 4.80 B. 6.00 C. 9.60 D.…