Textbook Question
Calculate the theoretical yield of product (in moles) for each initial amount of reactants.
3 Mn(s) + 2 O2(g) → Mn3O4(s)
a. 3 mol Mn, 2 mol O2
b. 4 mol Mn, 7 mol O2
c. 27.5 mol Mn, 43.8 mol O2
3760
views
1
rank
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 45
For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) a. 2.0 g Al, 2.0 g Cl2 b. 7.5 g Al, 24.8 g Cl2
Verified step by step guidance1
<Step 1: Determine the molar masses of the reactants and product. Calculate the molar mass of Al, Cl2, and AlCl3 using the periodic table.>
<Step 2: Convert the mass of each reactant to moles. Use the formula: moles = mass (g) / molar mass (g/mol) for both Al and Cl2.>
<Step 3: Identify the limiting reactant. Use the stoichiometry of the balanced equation to determine which reactant will be consumed first. Compare the mole ratio of Al to Cl2 from the balanced equation with the calculated moles.>
<Step 4: Calculate the theoretical yield of AlCl3. Use the moles of the limiting reactant and the stoichiometry of the balanced equation to find the moles of AlCl3 produced.>
<Step 5: Convert the moles of AlCl3 to grams. Use the formula: mass (g) = moles × molar mass (g/mol) to find the theoretical yield in grams.>
Related Practice
Textbook Question
Zinc sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2( g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
7102
views
1
comments
Textbook Question
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
8939
views
1
rank
Textbook Question
For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) c. 0.235 g Al, 1.15 g Cl2
643
views
Open Question
For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2(g) → TiF4(s) a. 5.0 g Ti, 5.0 g F2 b. 2.4 g Ti, 1.6 g F2
Textbook Question
For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2( g) → TiF4(s) c. 0.233 g Ti, 0.288 g F2
3446
views
1
rank