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 guidance

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.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using balanced chemical equations to determine how much of each substance is needed or produced. In this case, stoichiometry will help calculate the theoretical yield of aluminum chloride (AlCl3) based on the initial amounts of aluminum (Al) and chlorine (Cl2).

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the theoretical yield, as it dictates how much product can be produced from the available reactants. In the given question, one of the reactants (Al or Cl2) will limit the formation of AlCl3.

Theoretical Yield

Theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, assuming complete conversion and no losses. It is calculated using stoichiometric ratios derived from the balanced chemical equation. In this scenario, the theoretical yield of AlCl3 will be calculated based on the limiting reactant and the initial masses of Al and Cl2 provided.

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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?

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

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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

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