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Chapter 9: Problem 56

What do we mean by the actual yield of a reaction?

Short Answer

Expert verified
The actual yield of a reaction refers to the measured amount of one or more products that is really obtained from the experiment. It can be lower than the theoretical yield, which is the maximum possible amount of product that could be formed based on the balanced chemical equation. The actual yield is influenced by factors such as side reactions, incomplete reactions, or losses during the experimental process.

Step by step solution

01

Understanding chemical reactions and yield #-}

In a chemical reaction, reactants are converted into products. The amount of one or more products that is actually obtained from the reaction is called the yield. There are two types of yields, theoretical yield and actual yield. Theoretical yield is the maximum possible amount of product that could be formed from the limiting reactant, based on the equation, while the actual yield is the measured amount of product that is really obtained from the experiment. Actual yield can be lower than theoretical yield due to factors such as side reactions, incomplete reactions, or losses during the experimental process. It is important to distinguish between these two yields when discussing chemical reactions.

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Key Concepts

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

Chemical Reactions
Chemical reactions are processes where substances, known as reactants, are transformed into different substances, known as products. This involves breaking apart and forming new chemical bonds, leading to the creation of new chemical compounds. During this transformation, the mass is conserved according to the law of conservation of mass, which states that matter can neither be created nor destroyed in a chemical reaction. The equation representing a chemical reaction uses chemical formulas to show the reactants and products, thus providing a roadmap of the changes occurring during the reaction.
Theoretical Yield
Theoretical yield is the quantity of product predicted to form when a chemical reaction goes to completion. It is calculated based on the balanced chemical equation and assumes perfect conditions with no loss of material. To calculate the theoretical yield, one must first identify the limiting reactant because it dictates the maximum amount of product that can be formed. The calculation involves using stoichiometry; this requires the balanced chemical equation and molar masses of the reactants and products. Theoretical yield serves as a benchmark to measure the efficiency of a reaction, comparing actual results to the expected outcome.
Limiting Reactant
The limiting reactant is the substance in a chemical reaction that runs out first, limiting the amount of product that can be formed. Even if other reactants are present in excess, the reaction will stop once the limiting reactant is completely consumed. Identifying the limiting reactant is crucial for calculating the theoretical yield. To determine the limiting reactant, compare the mole ratio of the reactants used in the reaction to the ratio from the balanced equation. The reactant that provides the least amount of moles of product is the limiting reactant.
Experimental Process
The experimental process involves conducting a chemical reaction in a controlled setting to measure the quantities of reactants and products. It aims to determine the actual yield and compare it with the theoretical yield to assess the efficiency of the reaction. Several factors can affect the experimental process and decrease the actual yield below the theoretical yield. These include:
  • Side reactions, where unintended products are formed.
  • Incomplete reactions where not all reactants are converted into products.
  • Losses during product transfer, purification, or measurement errors.
To obtain accurate results, careful planning, precise measurement, and thorough execution of the experimental steps are crucial. Understanding these practical challenges helps in interpreting experimental data more effectively.

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Most popular questions from this chapter

Ethanol, the alcohol in beer and wine, has the molecular formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} .\) Calculate the mass percent of each element in ethanol.

A \(1.000-\mathrm{g}\) sample of a liquid is subjected to combustion analysis, yielding \(92.3 \% \mathrm{C}\) and \(7.7 \% \mathrm{H}\). It may or may not also contain oxygen. (a) What is the empirical formula for this compound? (b) The molar mass of this compound is determined to be about \(78 \mathrm{~g} / \mathrm{mol}\). What is the molecular formula for this compound?

Lead(II) sulfide reacts with hydrogen peroxide to give lead(II) sulfate as shown in the unbalanced chemical equation \(\mathrm{PbS}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{PbSO}_{4}+\mathrm{H}_{2} \mathrm{O}\) If \(63.2 \mathrm{~g}\) of \(\mathrm{PbS}\) is reacted with \(48.0 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}_{2}\) (a) Which is the limiting reagent? (b) How many grams of excess reactant remain after the reaction is complete?

Succinic acid, an intermediate in the metabolism of certain foods, has a molecular mass of \(118.1 \mathrm{~g} / \mathrm{mole}\). A \(1.926 \mathrm{~g}\) sample of succinic acid \(\left(\mathrm{H}_{x} \mathrm{Suc}\right)\) reacts with exactly \(1.25 \mathrm{~g}\) of \(\mathrm{NaOH}\) according to the following balanced equation: \(\mathrm{H}_{x} \mathrm{Suc}+x \mathrm{NaOH} \rightarrow \mathrm{Na}_{x} \mathrm{Suc}+x \mathrm{H}_{2} \mathrm{O}\) What is the value of \(x\) ?

Consider the unbalanced chemical equation \(\mathrm{As}_{4} \mathrm{~S}_{6}+\mathrm{O}_{2} \rightarrow \mathrm{As}_{4} \mathrm{O}_{6}+\mathrm{SO}_{2}\) (a) How many grams of \(\mathrm{O}_{2}\) are needed to react completely with \(58.9 \mathrm{~g}\) of \(\mathrm{As}_{4} \mathrm{~S}_{6}\) ? (b) If \(41.2 \mathrm{~g}\) of \(\mathrm{SO}_{2}\) is produced, what is the percent yield for the reaction?
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