aqueous sodium bromide Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce the theoretical yield of sodium bromide formed from the reaction of 0.81 g of hydrobromic acid and 0.17 g of sodium hydroxide? (NaBr) and liquid water (H₂O). What is
aqueous sodium bromide Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce the theoretical yield of sodium bromide formed from the reaction of 0.81 g of hydrobromic acid and 0.17 g of sodium hydroxide? (NaBr) and liquid water (H₂O). What is
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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![**Title: Theoretical Yield Calculation in a Chemical Reaction**
**Topic: Chemical Reactions and Stoichiometry**
**Overview:**
In this exercise, you will learn how to calculate the theoretical yield of a product from a chemical reaction involving hydrohalic acids and bases. The example below demonstrates the reaction between aqueous hydrobromic acid (HBr) and sodium hydroxide (NaOH).
**Problem Statement:**
Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H₂O). What is the theoretical yield of sodium bromide formed from the reaction of 6.18 g of hydrobromic acid and 0.17 g of sodium hydroxide? Round your answer to 2 significant figures.
**Calculation Method:**
1. **Write the balanced chemical equation:**
\[
\text{HBr} (aq) + \text{NaOH} (s) \rightarrow \text{NaBr} (aq) + \text{H}_{2}\text{O} (l)
\]
2. **Calculate the molar masses of the reactants:**
- Molar mass of HBr: \( \approx 80.91 \, \text{g/mol} \)
- Molar mass of NaOH: \( \approx 40.00 \, \text{g/mol} \)
3. **Convert mass of reactants to moles:**
Using the formula \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
- Moles of HBr:
\[
\text{Moles of HBr} = \frac{6.18 \, \text{g}}{80.91 \, \text{g/mol}} \approx 0.0764 \, \text{moles}
\]
- Moles of NaOH:
\[
\text{Moles of NaOH} = \frac{0.17 \, \text{g}}{40.00 \, \text{g/mol}} \approx 0.00425 \, \text{moles}
\]
4. **Determine the limiting reactant:**
- Compare the mole ratio of HBr and NaOH from the balanced equation](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F621954ed-ec20-4c07-b25b-e8811e0f0e49%2Febab7107-267e-48af-8a0d-e4a0f33de11b%2Foz9qd4t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Theoretical Yield Calculation in a Chemical Reaction**
**Topic: Chemical Reactions and Stoichiometry**
**Overview:**
In this exercise, you will learn how to calculate the theoretical yield of a product from a chemical reaction involving hydrohalic acids and bases. The example below demonstrates the reaction between aqueous hydrobromic acid (HBr) and sodium hydroxide (NaOH).
**Problem Statement:**
Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H₂O). What is the theoretical yield of sodium bromide formed from the reaction of 6.18 g of hydrobromic acid and 0.17 g of sodium hydroxide? Round your answer to 2 significant figures.
**Calculation Method:**
1. **Write the balanced chemical equation:**
\[
\text{HBr} (aq) + \text{NaOH} (s) \rightarrow \text{NaBr} (aq) + \text{H}_{2}\text{O} (l)
\]
2. **Calculate the molar masses of the reactants:**
- Molar mass of HBr: \( \approx 80.91 \, \text{g/mol} \)
- Molar mass of NaOH: \( \approx 40.00 \, \text{g/mol} \)
3. **Convert mass of reactants to moles:**
Using the formula \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
- Moles of HBr:
\[
\text{Moles of HBr} = \frac{6.18 \, \text{g}}{80.91 \, \text{g/mol}} \approx 0.0764 \, \text{moles}
\]
- Moles of NaOH:
\[
\text{Moles of NaOH} = \frac{0.17 \, \text{g}}{40.00 \, \text{g/mol}} \approx 0.00425 \, \text{moles}
\]
4. **Determine the limiting reactant:**
- Compare the mole ratio of HBr and NaOH from the balanced equation
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