What is the limiting reagent? and what is the mass of the leftover reagent? MgO(s)+H2S(g)=MgS(s)+H2O 22.7 g 17.9g

Pp

How many moles of sodium must react completely to produce 0.175 moles of sodium nitride in the equation                                                                  6Na + N2 --> 2Na3N   A 0.583 mol B 0.0292 mol C 0.525 mol D 0.175 mol  E 1.05 mol

What is the limiting reagent when 8.784 g of Fe is allowed to react with 39.78 g of water according to the reaction given below? Base your calculations on the yield of Fe2O3. 2 Fe + 3 H2O → Fe2O3 + 3 H2 a.  What is the limiting reactant? b.  What is the excess reagent? c.  What is the theoretical yield of Fe2O3?  g d.  How much of the excess reagent was used?  g e.  How much of the excess reagent was leftover?  g f.  The actual yield of iron (III) oxide was 1.981 g. What is the percent yield?  %

In the following balanced reaction 3.00 grams each of NO and Br2 are reacted together. How many grams of product can be produced? 2NO + Br2 ---> 2 NOBr

How many grams of fluorine (F2) are required to produce 10.0 grams of FeF3 from the balanced reaction shown? Given 1 mol F2 = 38 g 1 mol FeF3 = 113 g %3D %3D 2 Fe +3 F2→ 2 FeF3

How many grams of fluorine (F2) are required to produce 12.0 grams of FeF3 from the balanced reaction shown? Given 1 mol F2 = 38 g 1 mol FeF3 = 113 g %3D %3D 2 Fe +3 F2→ 2 FeF3

How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming the reaction has only 76.1% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g)

What mass of CO2 is produced when 100.0 g of Fe is produced?   118.2 g   150.0 g   133.7 g   What mass of Fe is produced when 100.0 g of Fe2O3 reacts?     93.71 g   69.94 g   125.2 g

How many moles of sodium azide (NaN3) are required to produce 0.235 mol N2? 2 NaN3(s) 2 Na(s) + 3 N2(g) O A) 0.157 mol B) 0.353 mol C) 0.0783 mol D) 0.470 mol