Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.

Ti(s) + 2 Cl₂(g) → TiCl₄(s)

a. 4 mol Ti, 4 mol Cl₂

b. 7 mol Ti, 17 mol Cl₂

c. 12.4 mol Ti, 18.8 mol Cl₂

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

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?

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?

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

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

Iron(III) oxide reacts with carbon monoxide according to the equation: Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) A reaction mixture initially contains 45.10 g Fe₂O₃ and 29.56 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Elemental phosphorus reacts with chlorine gas according to the equation: P₄(s) + 6 Cl₂( g) → 4 PCl₃(l) A reaction mixture initially contains 91.38 g P₄ and 262.6 g Cl₂. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O₂(g) → 2 MgO(s) When 13.1 g of Mg reacts with 13.6 g O₂, 12.4 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Urea (CH₄N₂O) is a common fertilizer that is synthesized by the reaction of ammonia (NH₃) with carbon dioxide: 2 NH₃(aq) + CO₂(aq) → CH₄N₂O(aq) + H₂O(l) In an industrial synthesis of urea, a chemist combines 149.4 kg of ammonia with 231.1 kg of carbon dioxide and obtains 172.3 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

Many computer chips are manufactured from silicon, which occurs in nature as SiO₂. When SiO₂ is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 177.4 kg of SiO₂ reacts with 100.1 kg of carbon to produce 71.2 kg of silicon. Determine the percent yield for the reaction.

Write the balanced chemical equation for the reaction of solid strontium with iodine gas.

Write the balanced chemical equation for the reaction of solid lithium with liquid water.

Write the balanced chemical equation for the reaction of solid potassium with liquid water.

Write the balanced equation for the reaction of hydrogen gas with bromine gas.

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 10.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Many home barbeques are fueled with propane gas (C₃H₈). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 37.8 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Aspirin can be made in the laboratory by reacting acetic anhydride (C₄H₆O₃) with salicylic acid (C₇H₆O₃) to form aspirin (C₉H₈O₄) and acetic acid (C₂H₄O₂). The balanced equation is: C₄H₆O₃ + C₇H₆O₃ → C₉H₈O₄ + C₂H₄O₂ In a laboratory synthesis, a student begins with 6.00 mL of acetic anhydride (density= 1.08 g/ mL) and 2.50 g of salicylic acid. Once the reaction is complete, the student collects 1.82 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield forthe reaction.

The combustion of liquid ethanol (C₂H₅OH) produces carbon dioxide and water. After 4.62 mL of ethanol (density = 0.789 g/mL) is allowed to burn in the presence of 15.55 g of oxygen gas, 3.72 mL of water (density = 1.00 g/mL) is collected. Determine the percent yield for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)

The reaction of NH₃ and O2 forms NO and water. The NO can be used to convert P₄ to P₄O₆, forming N₂ in the process. The P₄O₆ can be treated with water to form H₃PO₃, which forms PH₃ and H₃PO₄ when heated. Find the mass of PH₃ that forms from the reaction of 1.00 g of NH₃.

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO₂ from Fe₂O₃ and CO. Determine the mass of Fe₂O₃ required to form 910 kg of iron. Determine the amount of CO₂ that forms in this process.

A liquid fuel mixture contains 30.35% hexane (C₆H₁₄), 15.85% heptane (C₇H₁₆), and the rest octane (C₈H₁₈). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?

Titanium occurs in the magnetic mineral ilmenite (FeTiO₃), which is often found mixed with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO₃(s) + 3 Cl₂(g) + 3 C(s) → 3 CO(g) + FeCl₂(s) + TiCl₄(g) TiCl₄(g) + 2 Mg(s) → 2 MgCl₂(l) + Ti(s) Suppose that an ilmenite–sand mixture contains 22.8% ilmenite by mass and that the first reaction is carried out with a 90.8% yield. If the second reaction is carried out with an 85.9% yield, what mass of titanium can be obtained from 1.00 kg of the ilmenite– sand mixture?