In order to test the claim, your friend heats 5.0 g of CaCO3 strongly for 10 minutes over a Bunsen burner flame to cause the chemical reaction to occur. You can see gases coming off. After cooling, he measures the mass of the products formed and finds it is 2.9 grams. He’s highly confused, since he thought mass was being added , but it went down. Explain the change in mass of the products compared to the reactant.
In order to test the claim, your friend heats 5.0 g of CaCO3 strongly for 10 minutes over a Bunsen burner flame to cause the chemical reaction to occur. You can see gases coming off. After cooling, he measures the mass of the products formed and finds it is 2.9 grams. He’s highly confused, since he thought mass was being added , but it went down. Explain the change in mass of the products compared to the reactant.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 84QRT
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Question
In order to test the claim, your friend heats 5.0 g of CaCO3 strongly for 10 minutes over a Bunsen burner flame to cause the chemical reaction to occur. You can see gases coming off. After cooling, he measures the mass of the products formed and finds it is 2.9 grams. He’s highly confused, since he thought mass was being added , but it went down. Explain the change in mass of the products compared to the reactant.
*Figure 1: Setup at the start of the experiment showing 5.0 grams of CaCO₃.*
2. **During Heating**
- The CaCO₃ was heated strongly over a Bunsen burner. The image shows the test tube being heated, and gases can be seen forming and escaping from the test tube, indicating a decomposition reaction is occurring.
*Figure 2: CaCO₃ being heated with Bunsen burner flame; gas bubbles are visible in the test tube.*
3. **End (Mass: 2.9 grams)**
- After the reaction was completed and the product cooled, the final mass measured in the test tube was 2.9 grams.
*Figure 3: The setup at the end of the experiment showing a reduced mass of 2.9 grams.*
#### Explanation:
The observed decrease in mass can be explained by the chemical reaction that takes place when CaCO₃ is heated. The reaction is as follows:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
During heating, calcium carbonate decomposes to form calcium oxide (CaO) and carbon dioxide gas (CO₂). The carbon dioxide gas escapes into the atmosphere, resulting in a reduction in the mass of the solid product in the test tube. This explains the reduction from the initial mass of 5.0 grams to the final mass of 2.9 grams.
Your friend's confusion likely arises from a common misconception that mass should remain the same if no product is visibly lost. However,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46ade868-a4ca-4dcd-b69f-bba1f121fc8f%2Fd4b302cf-a11a-467c-adcf-c9242000b8fa%2Fjtt5f05_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Investigating the Mass Change During the Heating of Calcium Carbonate (CaCO₃)
To explore the effect of heating calcium carbonate (CaCO₃), your friend conducted an experiment by heating 5.0 grams of CaCO₃ strongly over a Bunsen burner for 10 minutes to induce a chemical reaction. During this process, gases were observed exiting the substance. After allowing the product to cool, the mass was measured and found to be 2.9 grams.
#### Experimental Steps:
1. **Start (Mass: 5.0 grams)**
- The initial mass of CaCO₃ placed in the test tube was 5.0 grams.
*Figure 1: Setup at the start of the experiment showing 5.0 grams of CaCO₃.*
2. **During Heating**
- The CaCO₃ was heated strongly over a Bunsen burner. The image shows the test tube being heated, and gases can be seen forming and escaping from the test tube, indicating a decomposition reaction is occurring.
*Figure 2: CaCO₃ being heated with Bunsen burner flame; gas bubbles are visible in the test tube.*
3. **End (Mass: 2.9 grams)**
- After the reaction was completed and the product cooled, the final mass measured in the test tube was 2.9 grams.
*Figure 3: The setup at the end of the experiment showing a reduced mass of 2.9 grams.*
#### Explanation:
The observed decrease in mass can be explained by the chemical reaction that takes place when CaCO₃ is heated. The reaction is as follows:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
During heating, calcium carbonate decomposes to form calcium oxide (CaO) and carbon dioxide gas (CO₂). The carbon dioxide gas escapes into the atmosphere, resulting in a reduction in the mass of the solid product in the test tube. This explains the reduction from the initial mass of 5.0 grams to the final mass of 2.9 grams.
Your friend's confusion likely arises from a common misconception that mass should remain the same if no product is visibly lost. However,
![**Decomposition of Calcium Carbonate**
**Introduction:**
The molecule \( \text{CaCO}_3 \) is what makes up eggshells, and it can decompose (break down) when heated strongly. This decomposition reaction is given by the equation:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
**Discussion:**
Your friend argues that the chemical equation doesn't follow the law of conservation of mass. He says, "Moles are not conserved since 1 mole of reactants produced 2 moles of product. This means the mass is higher in the end." You think he's wrong and want to explain and do an experiment to prove it.
**Explanation:**
The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. To address your friend's argument, it's important to understand that while the number of moles may differ, the total mass of the reactants must equal the total mass of the products. For the equation provided:
1. The reactant is 1 mole of \( \text{CaCO}_3 \).
2. The products are 1 mole of \( \text{CaO} \) and 1 mole of \( \text{CO}_2 \).
Even though the moles are different (1 mole of \( \text{CaCO}_3 \) decomposes into 2 moles of products), the mass is conserved because the molar masses account for this.
**Experiment:**
To prove the law of conservation of mass in this reaction, you can perform a simple experiment:
1. Weigh a clean and dry container.
2. Add a known mass of \( \text{CaCO}_3 \) (such as powdered eggshell) to the container and weigh it again.
3. Heat the \( \text{CaCO}_3 \) strongly until it decomposes completely into \( \text{CaO} \) and \( \text{CO}_2 \).
4. Allow the container to cool and weigh it.
You should observe that the mass of the \( \text{CaO} \) and the container is less than the initial mass of the \( \text{CaCO}_3 \) and the container because \( \text{CO}_2 \) is a gas and has escaped. By capturing and weighing the \( \text{CO}_](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46ade868-a4ca-4dcd-b69f-bba1f121fc8f%2Fd4b302cf-a11a-467c-adcf-c9242000b8fa%2F6zu615q_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Decomposition of Calcium Carbonate**
**Introduction:**
The molecule \( \text{CaCO}_3 \) is what makes up eggshells, and it can decompose (break down) when heated strongly. This decomposition reaction is given by the equation:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
**Discussion:**
Your friend argues that the chemical equation doesn't follow the law of conservation of mass. He says, "Moles are not conserved since 1 mole of reactants produced 2 moles of product. This means the mass is higher in the end." You think he's wrong and want to explain and do an experiment to prove it.
**Explanation:**
The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. To address your friend's argument, it's important to understand that while the number of moles may differ, the total mass of the reactants must equal the total mass of the products. For the equation provided:
1. The reactant is 1 mole of \( \text{CaCO}_3 \).
2. The products are 1 mole of \( \text{CaO} \) and 1 mole of \( \text{CO}_2 \).
Even though the moles are different (1 mole of \( \text{CaCO}_3 \) decomposes into 2 moles of products), the mass is conserved because the molar masses account for this.
**Experiment:**
To prove the law of conservation of mass in this reaction, you can perform a simple experiment:
1. Weigh a clean and dry container.
2. Add a known mass of \( \text{CaCO}_3 \) (such as powdered eggshell) to the container and weigh it again.
3. Heat the \( \text{CaCO}_3 \) strongly until it decomposes completely into \( \text{CaO} \) and \( \text{CO}_2 \).
4. Allow the container to cool and weigh it.
You should observe that the mass of the \( \text{CaO} \) and the container is less than the initial mass of the \( \text{CaCO}_3 \) and the container because \( \text{CO}_2 \) is a gas and has escaped. By capturing and weighing the \( \text{CO}_
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