If 3.42 g of K2PtCl4 and 1.61 g of NH3 give 2.08 g of cispla-tin (Problem 3.81), what is the percent yield of the reaction?

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Identify the balanced chemical equation for the reaction. The reaction involves K2PtCl4 and NH3 to form cisplatin (Pt(NH3)2Cl2).

Calculate the theoretical yield of cisplatin. First, determine the molar masses of K2PtCl4, NH3, and cisplatin (Pt(NH3)2Cl2).

Convert the given masses of K2PtCl4 and NH3 to moles using their respective molar masses.

Determine the limiting reactant by comparing the mole ratio of the reactants to the stoichiometry of the balanced equation.

Use the moles of the limiting reactant to calculate the theoretical yield of cisplatin in grams, then calculate the percent yield using the formula: \( \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \).

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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 determined using the formula: (actual yield / theoretical yield) x 100. A high percent yield indicates a more efficient reaction, while a low percent yield may suggest incomplete reactions or losses during the process.

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Percent Yield in Reactions

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to predict the amounts of substances consumed and produced in a reaction. Understanding stoichiometry is essential for determining the theoretical yield, which is the maximum amount of product that can be formed from given amounts of reactants.

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Stoichiometry Concept

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 of the product can be produced based on the initial quantities of reactants. The reactant in excess will remain after the reaction is complete.

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