Describe the relationship of ions and conductivity. Explain the concept of excess reactant, limiting reactant, theoretical yield, actual yield and % yield.
Describe the relationship of ions and conductivity. Explain the concept of excess reactant, limiting reactant, theoretical yield, actual yield and % yield.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Understanding the Relationship Between Ions and Conductivity**
Conductivity is a measure of a solution's ability to conduct electricity, which is facilitated by the presence of ions. Ions are charged particles formed when an ionic compound dissolves in a solvent, typically water. The mobility and concentration of these ions directly affect the conductivity of the solution. More ions result in higher conductivity, while fewer ions lower it.
**Key Concepts in Chemical Reactions:**
1. **Excess Reactant**: This is the reactant that remains after a chemical reaction has reached completion. It is available in a larger quantity than necessary to completely react with the limiting reactant.
2. **Limiting Reactant**: The reactant that is entirely consumed during a chemical reaction, thereby determining the maximum amount of product that can be formed. The limiting reactant controls the extent of the reaction.
3. **Theoretical Yield**: This is the maximum amount of product that could be formed from a given quantity of reactants, calculated based on stoichiometric ratios from the balanced chemical equation.
4. **Actual Yield**: The actual quantity of product obtained from a chemical reaction. It is often less than the theoretical yield due to factors like side reactions, incomplete reactions, or loss during recovery.
5. **Percent Yield**: A metric used to evaluate the efficiency of a reaction, calculated by the formula:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%
\]
Understanding these concepts is crucial in optimizing reactions and maximizing product formation in chemical processes.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf6c0134-f4f8-4f9a-a98d-fd2ffd62c181%2F418d63b2-3c62-4009-af7a-15f1b3988892%2F2obw1xk_processed.png&w=3840&q=75)
Transcribed Image Text:**Understanding the Relationship Between Ions and Conductivity**
Conductivity is a measure of a solution's ability to conduct electricity, which is facilitated by the presence of ions. Ions are charged particles formed when an ionic compound dissolves in a solvent, typically water. The mobility and concentration of these ions directly affect the conductivity of the solution. More ions result in higher conductivity, while fewer ions lower it.
**Key Concepts in Chemical Reactions:**
1. **Excess Reactant**: This is the reactant that remains after a chemical reaction has reached completion. It is available in a larger quantity than necessary to completely react with the limiting reactant.
2. **Limiting Reactant**: The reactant that is entirely consumed during a chemical reaction, thereby determining the maximum amount of product that can be formed. The limiting reactant controls the extent of the reaction.
3. **Theoretical Yield**: This is the maximum amount of product that could be formed from a given quantity of reactants, calculated based on stoichiometric ratios from the balanced chemical equation.
4. **Actual Yield**: The actual quantity of product obtained from a chemical reaction. It is often less than the theoretical yield due to factors like side reactions, incomplete reactions, or loss during recovery.
5. **Percent Yield**: A metric used to evaluate the efficiency of a reaction, calculated by the formula:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%
\]
Understanding these concepts is crucial in optimizing reactions and maximizing product formation in chemical processes.
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