One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(I) hydroxide from a solution containing rhodium() sulfate according to the following balanced chemical equation: Rh(SOah(aq) + 6N2OH(aq) - 2Rh(OH),(s) + 3Na,So,(aq) What is the theoretical yield of rhodium(Il) hydroxide from the reaction of 0.500 g of thodium(Il) sulfate with 1.100 g of sodium hydroxide? O 0.500 g O 0.156 g O 0.312 g O 141 g O 1.60 g
One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(I) hydroxide from a solution containing rhodium() sulfate according to the following balanced chemical equation: Rh(SOah(aq) + 6N2OH(aq) - 2Rh(OH),(s) + 3Na,So,(aq) What is the theoretical yield of rhodium(Il) hydroxide from the reaction of 0.500 g of thodium(Il) sulfate with 1.100 g of sodium hydroxide? O 0.500 g O 0.156 g O 0.312 g O 141 g O 1.60 g
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...
Related questions
Question
![### Chemical Reaction Questions
#### Question 1
One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following balanced chemical equation:
\[ \text{Rh}_2(\text{SO}_4)_3(\text{aq}) + 6\text{NaOH}(\text{aq}) \rightarrow 2\text{Rh(OH)}_3(\text{s}) + 3\text{Na}_2\text{SO}_4(\text{aq}) \]
What is the theoretical yield of rhodium(III) hydroxide from the reaction of 0.500 g of rhodium(III) sulfate with 1.100 g of sodium hydroxide?
- ○ 0.500 g
- ○ 0.156 g
- ○ 0.312 g
- ○ 1.41 g
- ○ 1.60 g
---
#### Question 2
If 48.0 g of \( \text{O}_2 \) is mixed with 48.0 g of \( \text{H}_2 \) and the mixture is ignited, what is the maximum mass of water that may be produced?
- ○ 48.0 g
- ○ 85.3 g
- ○ 54.0 g
- ○ 96 g
- ○ 432 g
### Explanation
Both questions involve stoichiometry, which is the calculation of reactants and products in chemical reactions.
In **Question 1**, the focus is on determining the theoretical yield of a product from given amounts of reactants. This involves:
1. Converting the mass of each reactant to moles.
2. Using the stoichiometric ratios from the balanced equation to determine the limiting reactant.
3. Calculating the theoretical yield of rhodium(III) hydroxide based on the limiting reactant.
In **Question 2**, the problem involves a combustion reaction with oxygen and hydrogen to form water. This requires:
1. Converting the mass of each reactant to moles.
2. Using the balanced equation for the combustion of hydrogen to determine the limiting reactant.
3. Calculating the maximum mass of water produced based on the limiting reactant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4b56968d-2846-4ccd-aa26-829d097f3532%2F8575d6d3-e79b-4e9f-9b12-c2801b1c7492%2Fzxdl3b5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Questions
#### Question 1
One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following balanced chemical equation:
\[ \text{Rh}_2(\text{SO}_4)_3(\text{aq}) + 6\text{NaOH}(\text{aq}) \rightarrow 2\text{Rh(OH)}_3(\text{s}) + 3\text{Na}_2\text{SO}_4(\text{aq}) \]
What is the theoretical yield of rhodium(III) hydroxide from the reaction of 0.500 g of rhodium(III) sulfate with 1.100 g of sodium hydroxide?
- ○ 0.500 g
- ○ 0.156 g
- ○ 0.312 g
- ○ 1.41 g
- ○ 1.60 g
---
#### Question 2
If 48.0 g of \( \text{O}_2 \) is mixed with 48.0 g of \( \text{H}_2 \) and the mixture is ignited, what is the maximum mass of water that may be produced?
- ○ 48.0 g
- ○ 85.3 g
- ○ 54.0 g
- ○ 96 g
- ○ 432 g
### Explanation
Both questions involve stoichiometry, which is the calculation of reactants and products in chemical reactions.
In **Question 1**, the focus is on determining the theoretical yield of a product from given amounts of reactants. This involves:
1. Converting the mass of each reactant to moles.
2. Using the stoichiometric ratios from the balanced equation to determine the limiting reactant.
3. Calculating the theoretical yield of rhodium(III) hydroxide based on the limiting reactant.
In **Question 2**, the problem involves a combustion reaction with oxygen and hydrogen to form water. This requires:
1. Converting the mass of each reactant to moles.
2. Using the balanced equation for the combustion of hydrogen to determine the limiting reactant.
3. Calculating the maximum mass of water produced based on the limiting reactant.
![### Example Problems on Percent Yield
**Problem 1: Sulfur Trioxide Production**
Sulfur trioxide (SO₃) is made from the oxidation of sulfur dioxide (SO₂), and the reaction is represented by the equation:
\[ 2 \text{SO}_2 + \text{O}_2 \rightarrow 2 \text{SO}_3 \]
A 22 g sample of SO₂ gives 18 g of SO₃. The percent yield of SO₃ is:
- 16%
- 100%
- 65%
- 28%
- 10%
**Problem 2: Silver Chloride Formation**
A 5.95 g sample of silver nitrate (AgNO₃) is reacted with barium chloride (BaCl₂) according to the equation:
\[ 2 \text{AgNO}_3 (\text{aq}) + \text{BaCl}_2 (\text{aq}) \rightarrow 2 \text{AgCl} (\text{s}) + \text{Ba(NO}_3)_2 (\text{aq}) \]
This reaction gives 4.00 g of AgCl. What is the percent yield of AgCl?
- 79.7%
- 100%
- 39.8%
- 67.2%
- 53.1%
### Explanation:
These problems involve calculating the percent yield, which is a measure of the efficiency of a chemical reaction. Percent yield is calculated using the formula:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]
**Graph/Diagram Explanation:**
There are no graphs or diagrams included in these problems. The illustration consists solely of text describing chemical reactions and options for possible answers to calculate the percent yield.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4b56968d-2846-4ccd-aa26-829d097f3532%2F8575d6d3-e79b-4e9f-9b12-c2801b1c7492%2Fvhodc1s_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Example Problems on Percent Yield
**Problem 1: Sulfur Trioxide Production**
Sulfur trioxide (SO₃) is made from the oxidation of sulfur dioxide (SO₂), and the reaction is represented by the equation:
\[ 2 \text{SO}_2 + \text{O}_2 \rightarrow 2 \text{SO}_3 \]
A 22 g sample of SO₂ gives 18 g of SO₃. The percent yield of SO₃ is:
- 16%
- 100%
- 65%
- 28%
- 10%
**Problem 2: Silver Chloride Formation**
A 5.95 g sample of silver nitrate (AgNO₃) is reacted with barium chloride (BaCl₂) according to the equation:
\[ 2 \text{AgNO}_3 (\text{aq}) + \text{BaCl}_2 (\text{aq}) \rightarrow 2 \text{AgCl} (\text{s}) + \text{Ba(NO}_3)_2 (\text{aq}) \]
This reaction gives 4.00 g of AgCl. What is the percent yield of AgCl?
- 79.7%
- 100%
- 39.8%
- 67.2%
- 53.1%
### Explanation:
These problems involve calculating the percent yield, which is a measure of the efficiency of a chemical reaction. Percent yield is calculated using the formula:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]
**Graph/Diagram Explanation:**
There are no graphs or diagrams included in these problems. The illustration consists solely of text describing chemical reactions and options for possible answers to calculate the percent yield.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps with 3 images
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY