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Ch.4 - Chemical Reactions and Chemical Quantities
All textbooksTro 5th EditionCh.4 - Chemical Reactions and Chemical QuantitiesProblem 44c
Chapter 4, Problem 44c

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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1
Determine the molar mass of each reactant and the product: Ti, F_2, and TiF_4.
Convert the mass of each reactant to moles using their respective molar masses.
Identify the limiting reactant by comparing the mole ratio of the reactants to the coefficients in the balanced chemical equation.
Use the moles of the limiting reactant to calculate the moles of TiF_4 produced, based on the stoichiometry of the reaction.
Convert the moles of TiF_4 to grams using its molar mass to find the theoretical yield.

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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 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 TiF4 based on the amounts of Ti and F2 provided.
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between the mass of reactants and products and the number of moles. To find the theoretical yield of TiF4, the molar masses of Ti and F2 must be calculated to determine how many moles of each reactant are present.
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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 TiF4 can be produced from the given amounts of Ti and F2.
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Related Practice
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

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Textbook Question

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?

Textbook Question

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?

Textbook Question

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.

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