When 22.5 g of O2 reacts with excess Mg only 42.5 g of MgO (MM=40.31 g/mol) is actually collected.  What is the percent yield for the reaction?                                                            2 Mg (s)   +   O2 (g)   à   2 MgO (s)

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows:  Cu2S(s) + O2(G) = 2 Cu (s) + SO2(g)  If the reaction of 0.530 kg of copper(I) sulfide with excess oxygen produces 0.290 kg of copper metal, what is the percent yield?  137% 39.9% 54.7% 274% 68.5%

What is the theoretical yield of HCI if 30.0 g of BCI3 and excess H20 are reacted according to the following balanced reaction? BC13(g) +3 H20(1) + H3BO3(s) + 3HCI(g) The following molar masses are: HCI = 36.46 g/mol BCI3 = 117.17 g/mol H2O = 18.02 g/mol

Mg(s) + 2 H2O(l) -> Mg(OH)2(aq) + H2(g) When 11.0g of Mg(s) reacts with excess water to produce 5.75g of Mg(OH)2 , what is the percent yield of the reaction?

Addition of NaOH to a Cu(NO3)2 solution results in the precipitation of Cu(OH)2.               2 NaOH     +     Cu(NO3)2     à     Cu(OH)2 (s)     +     2 NaNO3           If 10.00 g if NaOH is added to a solution that contains 25.00 g of Cu(NO3)2, what is the limiting reagent?  How many grams of Cu(OH)2 are produced?

If the percent yield for the following reaction is 75.0%, and 30.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

According to the following reaction, how many grams of oxygen gas are required for the complete reaction of 21.3 grams of hydrochloric acid?hydrochloric acid (aq) + oxygen (g)  water (l) + chlorine (g)

What is the maximum mass of H₂O that can be produced by combining 69.7 g of each reactant? 4 NH3(g) + 5O₂(g) 4 NO(g) + 6H₂O(g)

O 000 How many grams of HCl can react with 0.750 g of Al(OH)3 according the following balanced equation? Molar masses: Al(OH)3= 78.01 g, AICI3= 133.33 g, HCI= 36.46 g Al(OH)3(s) + 3 HCI (aq) --> AICI3(aq) + 3 H2O 3.85 g 1.05 g 0.0288 g 1.32 g

Calculate the number of moles of AI2O3 that are produced when 0.60 mol of Fe is produced in the following reaction: 2AI(s)+3FeO(s)—>3Fe(s)+AI2O3(s)