If 1.87 g of acetic acid (CH3COOH) reacts with 2.31 g of isopentyl alcohol (C5H12O) to give 2.96 g of isopentyl acetate (C7H14O2), what is the percent yield of the reaction?

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Identify the balanced chemical equation for the reaction: \[ \text{CH}_3\text{COOH} + \text{C}_5\text{H}_{12}\text{O} \rightarrow \text{C}_7\text{H}_{14}\text{O}_2 + \text{H}_2\text{O} \]

Calculate the molar mass of acetic acid (CH3COOH) and isopentyl alcohol (C5H12O) using the periodic table.

Determine the moles of acetic acid and isopentyl alcohol by dividing their given masses by their respective molar masses.

Identify the limiting reactant by comparing the mole ratio from the balanced equation to the moles calculated.

Calculate the theoretical yield of isopentyl acetate (C7H14O2) using the moles of the limiting reactant and convert it to grams. Then, use the formula for percent yield: \[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]

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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 calculation of reactants and products in chemical reactions based on the balanced chemical equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine how much of each substance is consumed or produced. Understanding stoichiometry is essential for determining theoretical yields and comparing them to actual yields in a reaction.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to the theoretical yield. It is expressed as a percentage and is calculated using the formula: (actual yield / theoretical yield) × 100%. This concept is crucial for evaluating how well a reaction proceeds and identifying any losses that may occur during the process.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule. Knowing the molar masses of reactants and products is vital for converting between grams and moles, which is necessary for stoichiometric calculations and determining theoretical yields in chemical reactions.

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