Limiting Reactant and Percent Yield

The chemical equation shows iron(III) phosphate reacting with sodium sulfate.

2FePO4 + 3Na2SO4 -->Fe2(SO4)3 + 2Na3PO4

What is the theoretical yield of Fe2(SO4)3 if 20.00 g of FePO4 reacts with an excess of Na2SO4?

26.52 g Fe2(SO4)3

Salicylic acid (C7H6O3) reacts with acetic anhydride (C4H6O3) to form acetylsalicylic acid (C9H8O4).

2C7H6O3(aq) + C4H6O3(aq)--> 2C9H8O4(aq) + H2O(l)

What is the limiting reactant if 70.0 g of C7H6O3 and 80.0 g of C4H6O3 react?

salicylic acid

Consider the balanced equation.

N2 + 3H2 -->2NH3

What is the percent yield of NH3 if the reaction of 26.3 g of H2 ACTUALLY produces 79.0 g of NH3? (Hint: calculate theoretical yield first!)

53.4%

Consider the combustion reaction for acetylene.

2C2H2(l) + 5O2(g) --> 4CO2(g) + 2H2O(g)

If the acetylene tank contains 37.0 mol of C2H2 and the oxygen tank contains 81.0 mol of O2, what is the limiting reactant for this reaction?

O2

The formula is used to calculate the percent yield of a reaction.

(actual yield/theoretical yield)x100%

What is used up first and stops a chemical reaction?

limiting reactant

Consider the balanced equation.

2HCl + Mg -->MgCl2 + H2

If 40.0 g of HCl react with an excess of magnesium metal, what is the theoretical yield of hydrogen?

1.11 g H2

The electrolysis of water forms H2 and O2.

2H2O --> 2H2 + O2

What is the percent yield of O2 if 10.2 g of O2 is ACTUALLY produced from the decomposition of 17.0 g of H2O? (Hint: calculate theoretical yield first!)

67.6%

Ammonia is produced by the following reaction.

3H2(g) + N2(g) -->2NH3(g)

When 7.00 g of hydrogen react with 70.0 g of nitrogen, ____________is considered the limiting reactant because_____

Hydrogen, 7.50 mol of hydrogen would be needed to consume the available nitrogen, and there is not enough (there is only 3.47 mol of hydrogen).

Consider the chemical equation.

CuCl2 + 2NaNO3 -->Cu(NO3)2 + 2NaCl

What is the percent yield of NaCl if 31.0 g of CuCl2 reacts with excess NaNO3 to ACTUALLY produce 21.2 g of NaCl? (Hint: calculate theoretical yield first!)

78.7%

Consider the balanced equation.

CuSO4 + Zn -->ZnSO4 + Cu

If 200.0 g of copper(II) sulfate react with an excess of zinc metal, what is the theoretical yield of copper?

1.253 g

The chemical equation shows how ammonia reacts with sulfuric acid to produce ammonium sulfate.

2NH3(aq) + H2SO4(aq) --> (NH4)2SO4(aq)

How many grams of ammonium sulfate can be produced if 60.0 mol of sulfuric acid react with an excess of ammonia?

3,970 g

Consider the following balanced equation:

2 H2 + O2 --> 2 H2O

What is the actual yield (in grams) of water produced if the reaction produced 23.8% of what it was supposed to when starting with 4.8 liters of oxygen and plenty of hydrogen? (Hint: calculate theoretical yield first!)

1.8 g H2O