Mole to Mole Ratios
Given the following decomposition reaction, calculate the moles of water produced from 2.97 mol of H2O2.
2 H2O2 (l) → 2 H2O (l) + O2 (g)
2.97 mol H2O
What is the mass of copper (II) nitrate that can be prepared from 2.38 g of copper metal?
Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s)
7.02 g Cu(NO3)2
Assuming constant conditions, how many milliliters of chlorine gas react to yield 3.45 L of dichlorine trioixde?
Cl2(g) + O2(g) → Cl2O3(g)
3450 mL Cl2
If 0.985 mole of nitrogen gas and 0.943 mol of oxygen gas react to produce nitrogen monoxide, what is the limiting reactant?
N2(g) + O2(g) → 2 NO(g)
O2
In the lab, 1.2 g of lead(II) oxide is collected. If the theoretical yield is 5.00 g, what is the percent yield?
24% yield
How many moles of oxygen are produced from the decomposition of 9.03 moles of LiClO3?
LiClO3(s) → LiCl(s) + O2(g)
13.5 mol O2
What is the mass of mercury that can be prepared from 6.48 g of cobalt metal?
Co(s) + HgCl2(aq) → CoCl3(aq) + Hg(l)
33.1 g Hg
Assuming constant conditions, how many milliliters of oxygen gas react to yield 540.0 mL of dinitrogen pentaoxide?
N2(g) + O2(g) → N2O5(g)
1350 mL O2
If 4.67 mol of hydrogen gas and 3.25 mol of oxygen gas react, what is the limiting reactant and how many moles of water are produced?
2 H2(g) + O2(g) → 2 H2O(l)
H2; 4.67 mol H2O
A 2.30 g sample of potassium bicarbonate is decomposed by heating. If the resulting potassium carbonate weighs 0.975 g and the calculated yield is 0.958 g, what is the percent yield?
102% yield
How many moles of Cl2 react with 89.4 moles of metallic iron, given the following reaction?
Fe(s) + Cl2(g) → FeCl3(s)
134 mol Cl2
How many grams of mercury (II) chloride react to give 5.39 g of Hg?
Co(s) + HgCl2(aq) → CoCl3(aq) + Hg(l)
7.30 g HgCl2
How many grams of mercury(II) oxide decompose to give 90.0 mL of oxygen gas at STP?
2 HgO(s) → 2 Hg(l) + O2(g)
1.74 g HgO
If 70.0 mL of nitrogen gas reacts with 45.0 mL of oxygen gas, what is the theoretical yield of N2O3 in liters?
N2(g) + O2(g) → N2O3(g)
0.0300 L N2O3
or 3.00*10-2 L N2O3
50.9 g of molten iron(II) oxide reacts with 10.4 g of magnesium. If a student collects 7.50 g of molten iron in a lab, what is the percent yield of the iron?
FeO(l) + Mg(l) → Fe(l) + MgO(s)
31.4% yield
How many moles of barium metal react to produce 0.125 mol of barium nitride?
Ba (s) + N2 (g) → Ba3N2 (s)
0.375 mol Ba
What is the mass of calcium phosphate that can be prepared from 3.90 g of Na3PO4?
Na3PO4(aq) + Ca(OH)2 (aq) → Ca3(PO4)2(s) + NaOH (aq)
3.69 g Ca3(PO4)2
How many grams of hydrogen peroxide decompose to give 49.5 mL of oxygen gas at STP?
H2O2(l) → H2O(l) + O2(g)
0.150 g H2O2
If 5.86 g of magnesium hydroxide reacts with 0.954 g of sulfuric acid, what is the theoretical yield of magnesium sulfate in grams?
Mg(OH)2(s) + H2SO4(l) → MgSO4(s) + H2O(l)
1.17 g MgSO4
If 5.05 g of cobalt reacted with 4.35 g of sulfur, and a student collected 0.989 g of cobalt(II) sulfide in the lab, what is the percent yield?
Co(s) + S(s) → CoS(s)
12.7% yield
How many moles of propane gas, C3H8, react with 4.32 moles of oxygen gas given the following combustion reaction?
C3H8(g) + O2(g) → CO2(g) + H2O(g)
0.864 mol C3H8
How many grams of calcium hydroxide react to give 2.54 g of Ca3(PO4)2?
Na3PO4(aq) + Ca(OH)2 (aq) → Ca3(PO4)2(s) + NaOH (aq)
1.82 g Ca(OH)2
How many milliliters of water are produced from the decomposition of 3.40 g of hydrogen peroxide, H2O2?
H2O2(l) → H2O(l) + O2(g)
2240 mL H2O
or 2.24*103 mL H2O
If 9.07 g of aluminum hydroxide reacted with 5.40 g of sulfuric acid, how much of the excess reactant is left over in grams?
Al(OH)3(s) + H2SO4(l) → Al2(SO4)3(aq) + H2O(l)
6.21 g Al(OH)3
If 9.58 g of ethane gas, C2H6, reacted with 8.67 g of oxygen gas, and 4.50 g of water was collected in the lab, what is the percent yield?
C2H6(g) + O2(g) → CO2(g) + H2O(g)
108% yield