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Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?

Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?

Chemistry
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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Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?

 

### Balancing Chemical Equations **Objective:** Balance each of the following chemical equations by adding coefficients where needed (even though we usually do not). 1. **Equation 1:** \[ \text{NaHCO}_3 (\text{s}) \rightarrow \text{NaOH} (\text{s}) + \text{CO}_2 (\text{g}) \] \[1 \quad\textcolor{gray}{\textbf{NaHCO}_3 (\text{s}) \rightarrow} \quad1 \quad \textcolor{gray}{\textbf{NaOH} (\text{s}) +} \quad1 \quad \textcolor{gray}{\textbf{CO}_2 (\text{g})} \] 2. **Equation 2:** \[ \text{NaHCO}_3 (\text{s}) \rightarrow \text{Na}_2\text{CO}_3 (\text{s}) + \text{CO}_2 (\text{g}) + \text{H}_2\text{O}(\text{g}) \] \[2 \quad\textcolor{gray}{\textbf{NaHCO}_3 (\text{s}) \rightarrow} \quad1 \quad \textcolor{gray}{\textbf{Na}_2\text{CO}_3 (\text{s}) +} \quad1 \quad \textcolor{gray}{\textbf{CO}_2 (\text{g}) +} \quad1 \quad \textcolor{gray}{\textbf{H}_2\text{O}(\text{g})} \] 3. **Equation 3:** \[ \text{NaHCO}_3 (\text{s}) \rightarrow \text{Na}_2\text{O} (\text{s}) + \text{CO}_2 (\text{g}) + \text{H}_2\text{O} (\text{g}) \] \[2 \quad\textcolor{gray}{\textbf{NaHCO}_3 (\text{s}) \rightarrow} \quad1 \quad \textcolor{gray}{\textbf{Na}_2\text{O} (\text{s}) +} \quad2 \quad \textcolor{gray}{\textbf{CO}_2 (\text{g})
Transcribed Image Text:### Balancing Chemical Equations **Objective:** Balance each of the following chemical equations by adding coefficients where needed (even though we usually do not). 1. **Equation 1:** \[ \text{NaHCO}_3 (\text{s}) \rightarrow \text{NaOH} (\text{s}) + \text{CO}_2 (\text{g}) \] \[1 \quad\textcolor{gray}{\textbf{NaHCO}_3 (\text{s}) \rightarrow} \quad1 \quad \textcolor{gray}{\textbf{NaOH} (\text{s}) +} \quad1 \quad \textcolor{gray}{\textbf{CO}_2 (\text{g})} \] 2. **Equation 2:** \[ \text{NaHCO}_3 (\text{s}) \rightarrow \text{Na}_2\text{CO}_3 (\text{s}) + \text{CO}_2 (\text{g}) + \text{H}_2\text{O}(\text{g}) \] \[2 \quad\textcolor{gray}{\textbf{NaHCO}_3 (\text{s}) \rightarrow} \quad1 \quad \textcolor{gray}{\textbf{Na}_2\text{CO}_3 (\text{s}) +} \quad1 \quad \textcolor{gray}{\textbf{CO}_2 (\text{g}) +} \quad1 \quad \textcolor{gray}{\textbf{H}_2\text{O}(\text{g})} \] 3. **Equation 3:** \[ \text{NaHCO}_3 (\text{s}) \rightarrow \text{Na}_2\text{O} (\text{s}) + \text{CO}_2 (\text{g}) + \text{H}_2\text{O} (\text{g}) \] \[2 \quad\textcolor{gray}{\textbf{NaHCO}_3 (\text{s}) \rightarrow} \quad1 \quad \textcolor{gray}{\textbf{Na}_2\text{O} (\text{s}) +} \quad2 \quad \textcolor{gray}{\textbf{CO}_2 (\text{g})
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