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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![Certainly, here is the transcription and explanation for the content:
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**Page 1 of 21**
**6.** What is the final molarity that would result if you diluted 180.0 mL of a 1.55 M HCl solution to a final volume of 500.0 mL?
**7.** Determine the volume of 1.5 M KI solution required for the reaction of 10.00 grams lead(II) nitrate.
**Reaction Equation:**
\[ \text{Pb(NO}_3\text{)}_2 + 2 \text{KI} \rightarrow \text{PbI}_2 + 2 \text{KNO}_3 \]
**8.** How many grams of KNO₃ are contained in 245 mL of 3.00 M KNO₃ solution?
**9.** If the combustion of 4.00 grams of magnesium results in the actual yield of 5.00 grams of magnesium oxide, what is the percent yield of the reaction?
**Reaction Equation:**
\[ 2\text{Mg(s)} + \text{O}_2\text{(g)} \rightarrow 2\text{MgO(s)} \]
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**Explanation of Reaction Equations:**
- **Reaction for Question 7:** Lead(II) nitrate reacts with potassium iodide to produce lead(II) iodide and potassium nitrate. The balanced equation shows that one mole of lead(II) nitrate reacts with two moles of potassium iodide.
- **Reaction for Question 9:** Magnesium reacts with oxygen to form magnesium oxide. The equation is balanced, indicating that two moles of magnesium and one mole of oxygen produce two moles of magnesium oxide.
This transcription provides an explanation for the chemical reactions mentioned and the associated questions related to molarity, volume, mass, and percent yield calculations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7cb7ab84-2909-44b4-aa38-afda86b9d9a5%2Fb5db2541-413d-4840-b704-b77457526b2c%2Fgvmxpin_processed.png&w=3840&q=75)
Transcribed Image Text:Certainly, here is the transcription and explanation for the content:
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**Page 1 of 21**
**6.** What is the final molarity that would result if you diluted 180.0 mL of a 1.55 M HCl solution to a final volume of 500.0 mL?
**7.** Determine the volume of 1.5 M KI solution required for the reaction of 10.00 grams lead(II) nitrate.
**Reaction Equation:**
\[ \text{Pb(NO}_3\text{)}_2 + 2 \text{KI} \rightarrow \text{PbI}_2 + 2 \text{KNO}_3 \]
**8.** How many grams of KNO₃ are contained in 245 mL of 3.00 M KNO₃ solution?
**9.** If the combustion of 4.00 grams of magnesium results in the actual yield of 5.00 grams of magnesium oxide, what is the percent yield of the reaction?
**Reaction Equation:**
\[ 2\text{Mg(s)} + \text{O}_2\text{(g)} \rightarrow 2\text{MgO(s)} \]
---
**Explanation of Reaction Equations:**
- **Reaction for Question 7:** Lead(II) nitrate reacts with potassium iodide to produce lead(II) iodide and potassium nitrate. The balanced equation shows that one mole of lead(II) nitrate reacts with two moles of potassium iodide.
- **Reaction for Question 9:** Magnesium reacts with oxygen to form magnesium oxide. The equation is balanced, indicating that two moles of magnesium and one mole of oxygen produce two moles of magnesium oxide.
This transcription provides an explanation for the chemical reactions mentioned and the associated questions related to molarity, volume, mass, and percent yield calculations.
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