Analysis: 1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations. 2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials: Trial 1: Trial 2: Trial 3: I
Analysis: 1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations. 2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials: Trial 1: Trial 2: Trial 3: I
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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Qs 1 and 2
![## Experiment Instructions
### Objective:
To measure the gas produced by the reaction between sodium hydrogen carbonate (NaHCO₃) and hydrochloric acid (HCl).
### Procedure:
1. Measure 5 separate quantities of sodium hydrogen carbonate (NaHCO₃), aiming for 0.5 g, 0.4 g, 0.3 g, 0.2 g, and 0.1 g. Record the exact masses in Table 2.1.
2. Obtain about 40 mL of 0.7 M HCl in a 50 mL beaker.
3. Add 2 drops of indicator to each flask and observe any color change.
4. Set up a gas collection apparatus as demonstrated by the TA.
5. Collect 5.0 mL of hydrochloric acid into the syringe.
6. Inject the acid and allow to react. (Account for this volume to measure the gas produced accurately.)
### Reaction Equation:
\[ \text{HCl(aq)} + \text{NaHCO}_3\text{(s)} \rightarrow \text{CO}_2\text{(g)} + \text{H}_2\text{O(l)} + \text{NaCl(aq)} \]
**Equation 2.1**
---
### Data
#### Table 2.1
| Flask | Volume of 0.700 M HCl (mL) | Mole HCl | Mass of NaHCO₃ (g) | Mole NaHCO₃ (84.0 g/mol) |
|-------|----------------------------|----------|--------------------|--------------------------|
| 1 | 5.00 | | 0.1 | |
| 2 | 5.00 | | 0.3 | |
| 3 | 5.00 | | 0.5 | |
---
### Results
#### Table 2.2
| Flask | Color of Solution After Reaction | Volume of Gas Produced (mL) | Solid Residue (Y/N) | What Reactant was Limiting (Used Up)? | What Reactant was in Excess (Some Left Over)? |
|-------|----------------------------------|-----------------------------|---------------------|---------------------------------------|-----------------------------------------------|
| 1 | Light pink | 29 | N | NaHCO](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff787f97c-9dc4-4f39-97ba-c4c8bbc1d69b%2F168e0019-4338-4623-a435-66585326e687%2Fuxx17np_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Experiment Instructions
### Objective:
To measure the gas produced by the reaction between sodium hydrogen carbonate (NaHCO₃) and hydrochloric acid (HCl).
### Procedure:
1. Measure 5 separate quantities of sodium hydrogen carbonate (NaHCO₃), aiming for 0.5 g, 0.4 g, 0.3 g, 0.2 g, and 0.1 g. Record the exact masses in Table 2.1.
2. Obtain about 40 mL of 0.7 M HCl in a 50 mL beaker.
3. Add 2 drops of indicator to each flask and observe any color change.
4. Set up a gas collection apparatus as demonstrated by the TA.
5. Collect 5.0 mL of hydrochloric acid into the syringe.
6. Inject the acid and allow to react. (Account for this volume to measure the gas produced accurately.)
### Reaction Equation:
\[ \text{HCl(aq)} + \text{NaHCO}_3\text{(s)} \rightarrow \text{CO}_2\text{(g)} + \text{H}_2\text{O(l)} + \text{NaCl(aq)} \]
**Equation 2.1**
---
### Data
#### Table 2.1
| Flask | Volume of 0.700 M HCl (mL) | Mole HCl | Mass of NaHCO₃ (g) | Mole NaHCO₃ (84.0 g/mol) |
|-------|----------------------------|----------|--------------------|--------------------------|
| 1 | 5.00 | | 0.1 | |
| 2 | 5.00 | | 0.3 | |
| 3 | 5.00 | | 0.5 | |
---
### Results
#### Table 2.2
| Flask | Color of Solution After Reaction | Volume of Gas Produced (mL) | Solid Residue (Y/N) | What Reactant was Limiting (Used Up)? | What Reactant was in Excess (Some Left Over)? |
|-------|----------------------------------|-----------------------------|---------------------|---------------------------------------|-----------------------------------------------|
| 1 | Light pink | 29 | N | NaHCO
Transcribed Image Text:**Analysis:**
1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations.
2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials:
- Trial 1:
- Trial 2:
- Trial 3:
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