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Chapter 11: Problem 85

Can the percent yield of a chemical reaction be more than 100\(\% ?\) Explain your answer.

Short Answer

Expert verified
No, the percent yield of a chemical reaction cannot be more than 100%. This is because the theoretical yield sets the maximum amount of product that can be obtained from a reaction given the limiting reactant. If the actual yield were to exceed the theoretical yield, it would suggest an error in either the reaction stoichiometry or the measurement of the actual yield. Therefore, a yield exceeding 100% is indicative of erroneous calculations or measurements, as it implies the production of more product than what is chemically possible from the limiting reactant.

Step by step solution

01

Defining Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual yield (the amount of product obtained) to the theoretical yield (the maximum amount of product that can be produced from the limiting reactant) multiplied by 100%. The equation for percent yield is: \[ \% \, yield = \frac{actual \, yield}{theoretical \, yield} \times 100\%\]
02

Understanding Limiting Reactants

In a chemical reaction, the limiting reactant is the substance that is completely consumed and determines the maximum amount of product that can be formed. The other reactants are present in excess and do not affect the yield directly.
03

Considering a Percent Yield Over 100%

For the percent yield to be more than 100%, the actual yield would need to be greater than the theoretical yield. This implies that more product is obtained from the limiting reactant than what is theoretically possible based on the stoichiometry of the reaction.
04

Explanation

It is not possible for the percent yield of a chemical reaction to be more than 100%. This is because the actual yield cannot surpass the theoretical yield, as the limiting reactant determines the maximum amount of product that can be formed. If more product were formed than what is theoretically expected, it would mean that either there is an error in the reaction stoichiometry or in the measurement of the actual yield.

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Key Concepts

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

Chemical Reaction
In chemistry, a chemical reaction is a process where substances, known as reactants, transform into different substances called products. These transformations are critical to many natural phenomena and industrial processes. During a chemical reaction, bonds between atoms in the reactants are broken and new bonds are formed in the products. This process often results in changes in energy.
  • Reactants: The initial substances in a chemical reaction.
  • Products: The substances produced by the chemical reaction.
The nature of chemical reactions is governed by the laws of chemistry, such as conservation of mass and energy. This means that the total mass and energy before and after a reaction must be equal.
Limiting Reactants
The limiting reactant is an essential idea in chemistry for predicting how much product a reaction can produce. It is the reactant that gets completely used up during the reaction. Why is it called 'limiting'? Because it limits the amount of product formed. Once this reactant is fully consumed, the reaction cannot proceed further. To identify the limiting reactant in a chemical equation, you compare the amount of reactants available based on the balanced equation. Here's why it's important:
  • It directly determines the theoretical yield of the reaction.
  • It ensures efficient use of resources in industrial reactions.
  • It helps in calculating the perfect amounts for reactions in labs or industry.
Theoretical Yield
Theoretical yield refers to the maximum amount of product that could be formed from a given amount of limiting reactant, according to the stoichiometry of the balanced chemical equation. It assumes perfect conditions where all reactants are converted into products, with no loss. Calculation of the theoretical yield requires:
  • Balanced chemical equation.
  • Molar masses of reactants and products.
  • Identification of the limiting reactant.
However, in real-world conditions, reactions rarely achieve their theoretical yield due to factors like incomplete reactions, side reactions, or practical losses during handling and measurement.
Actual Yield
The actual yield is the quantity of product actually obtained from a chemical reaction. It is usually less than the theoretical yield due to various practical factors. Achieving actual yield involves carrying out the chemical reaction under realistic experimental conditions. Common reasons for a lower actual yield include:
  • Incomplete reactions where not all reactants are converted to products.
  • Side reactions that produce different unwanted products.
  • Losses during the process of isolation and purification of products.
Understanding both theoretical and actual yields is crucial for calculating the percent yield, which evaluates the efficiency of a particular reaction.

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Most popular questions from this chapter

Lithium reacts spontaneously with bromine to produce lithium bromide. Write the balanced chemical equation for the reaction. If 25.0 g of lithium and 25.0 g of bromine are present at the beginning of the reaction, determine a. the limiting reactant. b. the mass of lithium bromide produced. c. the excess reactant and the excess mass.

Challenge For each of the following, balance the chemical equation; interpret the equation in terms of particles, moles, and mass; and show that the law of conservation of mass is observed. a) ____\(\mathrm{Na}(\mathrm{s})+\)____\(\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow\) ____\(\mathrm{NaOH}(\mathrm{aq})+\) ____\(\mathrm{H}_{2}(\mathrm{g})\) b) ____\(Z n(s)+\) ____\(\mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow\) ____\(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\) ____\(\mathrm{H}_{2} \mathrm{O}(\mathrm{l})\)

To extract gold from its ore, the ore is treated with sodium cyanide solution in the presence of oxygen and water. \(4 \mathrm{Au}(\mathrm{s})+8 \mathrm{NaCN}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(1) \rightarrow\) \(4 \mathrm{NaAu}(\mathrm{CN})_{2}(\mathrm{aq})+4 \mathrm{NaOH}(\mathrm{aq})\) a. Determine the mass of gold that can be extracted if 25.0 \(\mathrm{g}\) of sodium cyanide is used. b. If the mass of the ore from which the gold was extracted is \(150.0 \mathrm{g},\) what percentage of the ore is gold?

Describe how a mole ratio is correctly expressed when it is used to solve a stoichiometric problem.

Aluminum hydroxide \(\left(\mathrm{Al}(\mathrm{OH})_{3}\right)\) is often present in antacids to neutralize stomach acid \((\mathrm{HCl})\) The reaction occurs as follows: \(\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s})+3 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{D}) .\) If 14.0 \(\mathrm{g}\) of \(\mathrm{Al}(\mathrm{OH})_{3}\) is present in an antacid tablet, determine the theoretical yield of \(\mathrm{AlCl}_{3}\) produced when the tablet reacts with \(\mathrm{HCl}\)
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