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Chapter 11: Problem 86

What relationship is used to determine the percent yield of a chemical reaction?

Short Answer

Expert verified
The percent yield of a chemical reaction is determined using the relationship: Percent Yield = \(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\) 脳 100, where actual yield is the obtained product quantity and theoretical yield is the maximum possible product amount based on stoichiometry. This formula measures the efficiency of a reaction by comparing the actual yield to the theoretical yield.

Step by step solution

01

Understand the theoretical yield and actual yield

Theoretical yield is the maximum amount of product that can be formed from a given amount of reactants in a chemical reaction. It is based on the stoichiometry of the balanced chemical equation. On the other hand, actual yield is the quantity of product that is obtained after the completion of a chemical reaction. Actual yield is often less than the theoretical yield due to side reactions, incomplete reactions, or loss of product during purification.
02

Define percent yield

Percent yield is a measure of the efficiency of a chemical reaction. It is the ratio of the actual yield to the theoretical yield, expressed as a percentage. It gives an idea of how much product is obtained compared to the maximum possible amount.
03

Write the formula for percent yield

To calculate the percent yield, we need to divide the actual yield by the theoretical yield, and then multiply by 100 to express it as a percentage. The formula for percent yield is as follows: Percent Yield = \(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\) 脳 100 Now, you can use this relationship to calculate the percent yield of any chemical reaction, given the actual and theoretical yields.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Theoretical Yield
The theoretical yield represents the maximum amount of product that can be generated from a given quantity of reactants in a chemical reaction. This calculation is based on the assumption that every single reactant particle successfully reacts, following the stoichiometry outlined in the balanced chemical equation.
It doesn't consider any practical limitations or inefficiencies that might occur in a real-world reaction.

Some key points to remember about theoretical yield:
  • It is an ideal value, assuming perfect conditions.
  • It is determined using stoichiometric calculations.
  • It helps in assessing how efficient the reaction is when compared to actual results.
Theoretical yield is crucial when planning experiments, as it provides a maximum amount of product one can expect.
Actual Yield
The actual yield is the quantity of product that is obtained after a chemical reaction is carried out. In real-life scenarios, the actual yield is often less than the theoretical yield. This discrepancy is due to several factors, such as side reactions that consume some of the reactants or form other products, incomplete reactions, and losses during the recovery or purification process.
Understanding actual yield helps chemists evaluate the efficiency and the practical aspects of their reactions.

Here are some factors affecting actual yield:
  • Impurities in reactants: Affect the reactivity and final product.
  • Operator errors: Mistakes during the measurement or process can reduce yield.
  • External conditions: Temperature and pressure changes affecting the reaction rate.
By evaluating the actual yield, scientists can make necessary adjustments to improve the reaction process.
Stoichiometry
Stoichiometry is the fundamental concept of chemistry that involves the calculation of reactants and products in a chemical reaction. It is based on the laws of conservation of mass and the premise that atoms are neither created nor destroyed during a chemical reaction. Stoichiometry allows chemists to predict the amounts of substances consumed and produced in reactions.
It can be thought of as the mathematical foundation underpinning the calculations for theoretical yield.

Essential elements of stoichiometry include:
  • Writing balanced chemical equations.
  • Using mole ratios as a conversion factor.
  • Predicting yields and reactant needs based on known quantities.
By mastering stoichiometry, one can efficiently determine how much of each reactant is needed and what quantity of product will form.
Chemical Reaction Efficiency
Chemical reaction efficiency is assessed by calculating the percent yield. It reflects how effective a reaction is by comparing the actual yield to the theoretical yield. The percent yield provides a straightforward metric to evaluate the success of a reaction in practical terms.
To compute percent yield:
  • Use the formula:
    Percent Yield = \( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100 \)
  • Ensure the units for actual and theoretical yields are consistent.
  • The closer the percent yield is to 100%, the more efficient the reaction.
Understanding percent yield enables scientists and students to determine how much of the initial material was converted into the desired product, facilitating improvements in experimental conditions.

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Most popular questions from this chapter

Upon heating, calcium carbonate \(\left(\mathrm{CaCO}_{3}\right)\) decomposes to calcium oxide \((\mathrm{CaO})\) and carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) a. Determine the theoretical yield of \(\mathrm{CO}_{2}\) if 235.0 \(\mathrm{g}\) of \(\mathrm{CaCO}_{3}\) is heated. b. What is the percent yield of \(\mathrm{CO}_{2}\) if 97.5 \(\mathrm{g}\) of \(\mathrm{CO}_{2}\) is collected?

Air Pollution Nitrogen oxide, which is present in urban air pollution, immediately converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen oxide. b. What mole ratio would you use to convert from moles of nitrogen oxide to moles of nitrogen dioxide?

Solid silicon dioxide, often called silica, reacts with hydrofluoric acid (HF) solution to produce the gas silicon tetrafluoride and water. a. Write the balanced chemical equation for the reaction. b. List three mole ratios, and explain how you would use them in stoichiometric calculations.

Ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) also known as grain alcohol, can be made from the fermentation of sugar \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) The unbalanced chemical equation for the reaction is shown below. ___ \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} \rightarrow\) ___ \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}+\)___ \(\mathrm{CO}_{2}\) Balance the chemical equation and determine the mass of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) produced from 750 \(\mathrm{g}\) of \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

Challenge Sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) is formed when sulfur dioxide (SO_{2} ) reacts with oxygen and water. a. Write the balanced chemical equation for the reaction. b. How many moles of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is produced from 12.5 \(\mathrm{moles}\) of \(\mathrm{SO}_{2} ?\) c. How many moles of \(\mathrm{O}_{2}\) are needed?
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