True or false to calculate the percent yield of a reaction, the correct formula is percent yield = actual yield/ predicted yield x 100 %

consider the following balanced equation. N2O4(l) + 2 N2H4(l)  →  3 N2(g) + 4 H2O(g) Determine the theoretical yield  in gram of nitrogen, N2 , that can be formed from  60.0 g N2O4 and  55.0 g N2H4  ? If the actual experimental yield for N2 is 37.2 g, what is the percent yield of N2? Some possibly useful molar masses are as follows:  N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol, N2 = 28.00 g/mol (Hint: the theoretical yield is determined from the limiting reactant. So, you have to find how much gram of N2 is produced from 50.0 g of N2O2 and how much gram of N2 is produced from 45.0 g of N2H4.  The one, either the N2O4 or N2H4 , produces the least gram of N2 is called the limiting reactant and the amount of N2 produced  from the limiting reactant is called  the theoretical yield.   Finally, % yield = (Actual / theoretical) x 100 =

NaCI(s) + H,SO (aq) →_ Na,so,(s) + HCI(g) - Balance the equation above. If 32.5 g NaCl and 24.5 g sulfuric acid are reacted, and 15.5 g HCl is produced, what is the percent yield for this reaction? HINT: Determine the limiting reactant first, and use this reactant to calculate the theoretical yield   z

Consider the reaction. 2 Pb(s) + 0,(g) –→ 2 PbO(s) An excess of oxygen reacts with 451.4 g of lead, forming 322.5 g of lead(II) oxide. Calculate the percent yield of the reaction. percent yield: % * TOOLS x10