Question

22) Given that 4 NH3 +50,-- 4 NO:6 HO.if 3.00 mol NHy were made to react with excess of oxygen gas, the amount of H2O formed would be: A) 4.50 mol B) 2.00 mol. C) 6.00 mol. D) 3.00 mol. E) none of the above 23) Which of the following statements is FALSE? A) The actual yield is the amount of product actually produced by a chemical reaction. B) The percent yield - Actual Yield Theoretical Yield"100 C) The limiting reactant is completely consumed in a chemical reaction D) The theoretical yield is the amount of product that can be made based on the amount of limiting reagent. E) All of the above are true statements. 24) Consider the following generic chemical equation: 2W.3X -- 3Y+Z When 5 units of W and 6 units of X are allowed to react, the limiting reactant would be: A) X B) W C) Y D) Z E) There is no limiting reactant in this situation. 25) A balanced chemical equation used to prepare ammonium carbonate, (NH4)2CO3, is: 2 NH3 +CO2 +H20 -- (NH4)2CO3 Which choice of reactant quantities shown below would result in the greatest amount of ammonium carbonate being formed? A) React 2 moles NH3, 8 moles CO2, and 8 moles H2O B) React 2 moles NH3 , 1 mole CO2 and 1 mole H20 C) React 4 moles NH3 , 1 mole CO2, and 2 moles H2O D) React 4 moles NH3,2 moles CO2 and 2 moles H20 E) none of the above 26) 26) What is the theoretical yield of a reaction if 25.0 grams of product were actually produced from a reaction that has a 88% yield? A) 3.52 B) 28.4 C) 352 D) 22.0 E) none of the above

Answer 1

Answer (22) 4NH3+5O2--------> 4NO+6H2O

As per the above reaction

4 mole of NH3 produces = 6 mole of H2O

1 mole of NH3 will produce = 6/4 mole of H2O

3 mole of NH3 will produce = (6/4)*3=4.50 moles of H2O (option A)