I am not sure what the products of the reactions should be. 1) Get two test tubes and a wooden test tube rack. Into one test tube, add about 2 mL of 6 M HCl. Place a single piece of copper metal into the other test tube. Write the appearance of each below and then pour the acid over the copper. Observe what happens and write a balanced net ionic equation on your data sheet. need help with question 1-3
I am not sure what the products of the reactions should be. 1) Get two test tubes and a wooden test tube rack. Into one test tube, add about 2 mL of 6 M HCl. Place a single piece of copper metal into the other test tube. Write the appearance of each below and then pour the acid over the copper. Observe what happens and write a balanced net ionic equation on your data sheet. need help with question 1-3
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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Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
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I am not sure what the products of the reactions should be.
1) Get two test tubes and a wooden test tube rack. Into one test tube, add about 2 mL of 6 M HCl. Place a single piece of copper metal into the other test tube. Write the appearance of each below and then pour the acid over the copper. Observe what happens and write a balanced net ionic equation on your data sheet.
need help with question 1-3
![**Chemistry I Laboratory Manual, 2021 Revision**
**Laboratory Report**
**Name:** Edgar Domingues
**Date:** 10/21/2022
**Partner's Name:** Daniel Diaz
**Instructor's Initials:** [Blank]
---
### Part A: Redox Equations Involving Copper and Acids
| Experiment Number | Substance Oxidized | Substance Reduced | Observations | [Balanced Net Ionic] Equation |
|-------------------|--------------------|-------------------|--------------|-------------------------------|
| 1 | - | - | HCl: clear liquid<br>Cu: bronze-like metal<br>No reaction | Product = clear liquid & some metal |
**Note:**
- **Cu(s) + HCl(aq) → No Reaction**
- Copper is less reactive than hydrogen, so it wouldn't be able to displace it. No transfer of electrons, so no redox reaction.
| 2 | Cu | HNO₃ | HNO₃: clear<br>Cu: bronze-like metal<br>Product = bubbles started to come from the copper | [Blank] |
| 3 | Cu | HNO₃ | HNO₃: clear<br>Cu: bronze-like metal<br>Product = green solution and brown gas | **Cu(s) + HNO₃ → Cu²⁺ + NO₂** |
**Note:**
- In Experiment 3, copper reacts with nitric acid, producing a green solution and brown gas.
This table displays observations and reactions of copper with different acids, highlighting the principles of reactivity and electron transfer in redox reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe7a54da2-bb36-4266-99d7-672b4d4e9da7%2F45313501-1d84-466c-a83a-f88e7def7bb7%2Fv5qcx7n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemistry I Laboratory Manual, 2021 Revision**
**Laboratory Report**
**Name:** Edgar Domingues
**Date:** 10/21/2022
**Partner's Name:** Daniel Diaz
**Instructor's Initials:** [Blank]
---
### Part A: Redox Equations Involving Copper and Acids
| Experiment Number | Substance Oxidized | Substance Reduced | Observations | [Balanced Net Ionic] Equation |
|-------------------|--------------------|-------------------|--------------|-------------------------------|
| 1 | - | - | HCl: clear liquid<br>Cu: bronze-like metal<br>No reaction | Product = clear liquid & some metal |
**Note:**
- **Cu(s) + HCl(aq) → No Reaction**
- Copper is less reactive than hydrogen, so it wouldn't be able to displace it. No transfer of electrons, so no redox reaction.
| 2 | Cu | HNO₃ | HNO₃: clear<br>Cu: bronze-like metal<br>Product = bubbles started to come from the copper | [Blank] |
| 3 | Cu | HNO₃ | HNO₃: clear<br>Cu: bronze-like metal<br>Product = green solution and brown gas | **Cu(s) + HNO₃ → Cu²⁺ + NO₂** |
**Note:**
- In Experiment 3, copper reacts with nitric acid, producing a green solution and brown gas.
This table displays observations and reactions of copper with different acids, highlighting the principles of reactivity and electron transfer in redox reactions.
Transcribed Image Text:**Redox Reactions**
| Chemical Substance | Appearance |
|--------------------|------------|
| CO₂ | colorless gas |
| C₂O₄²⁻ | colorless in solution |
| Cu metal | "copper-colored" metal |
| Cu²⁺ | varies from blue to green in aqueous solution |
| NO₃⁻ | colorless in aqueous solution |
| NO₂ | red-brown gas |
| NO₂⁻ | colorless in aqueous solution |
| NO | colorless gas |
| MnO₄⁻ | purple in aqueous solution |
| MnO₂ | muddy black precipitate |
| Mn²⁺ | light pink to colorless in aqueous solution |
| Cr₂O₇²⁻ | orange in aqueous solution |
| Cr³⁺ | dark green, blue gray, or purple depending on complex in aqueous solution |
| I₂ | red brown solid, violet vapor, yellow to brown in solution |
| I⁻ | colorless in aqueous solution |
| Fe³⁺ | red-brown in basic solution, colorless in acidic solution |
| Fe²⁺ | light green to colorless in aqueous solution |
**Part A: Reactions of Copper Metal with Acids (your instructor may wish to demonstrate this)**
1. Get two test tubes and a wooden test tube rack. Into one test tube, add about 2 mL of 6 M HCl. Place a single piece of copper metal into the other test tube. Write the appearance of each below and then pour the acid over the copper. Observe what happens and write a balanced net ionic equation on your data sheet.
2. Get two more test tubes and place them into the wooden test tube rack. Into one test tube, add about 2 mL of 6 M HNO₃. Place a single piece of copper metal into the other test tube. Write the appearance of each on the data sheet. *In the fume hood*
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