Consider the reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) + 2 Cl₂(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl₂ form from the reaction mixture that produces the greatest amount of products?

Consider the reaction: 2 CH₃OH(g) + 3 O₂(g) → 2 CO₂(g) + 4 H₂O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO₂ molecules form from the reaction mixture that produces the greatest amount of products?

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?

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 22.55 g Fe₂O₃ and 14.78 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 45.69 g P₄ and 131.3 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 10.1 g of Mg reacts with 10.5 g O₂, 11.9 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 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 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, 155.8 kg of SiO₂ reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the percent yield for the reaction.

Calculate the molarity of each solution.

a. 3.25 mol of LiCl in 2.78 L solution

b. 28.33 g C₆H₁₂O₆ in 1.28 L of solution

Calculate the molarity of each solution.

c. 32.4 mg NaCl in 122.4 mL of solution

Calculate the molarity of each solution. a. 0.38 mol of LiNO₃ in 6.14 L of solution b. 72.8 g C₂H₆O in 2.34 L of solution c. 12.87 mg KI in 112.4 mL of solution

What is the molarity of NO₃^– in each solution? a. 0.150 M KNO₃ b. 0.150 M Ca(NO₃)₂ c. 0.150 M Al(NO₃)₃

what is the molarity of Cl^- in each solution? a. 0.200 M NaCl

What is the molarity of Cl^- in each solution? b. 0.150 M SrCl₂

what is the molarity of Cl^- in each solution? c. 0.100 M AlCl₃

How many moles of KCl are contained in each solution? a. 0.556 L of a 2.3 M KCl solution

How many moles of KCl are contained in each solution? b. 1.8 L of a 0.85 M KCl solution

How many moles of KCl are contained in each solution? c. 114 mL of a 1.85 M KCl solution

What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? a. 0.45 mol ethanol

What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? b. 1.22 mol ethanol