Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of water formed from the reaction of 2.10g of ethane and 15.1g of oxygen gas? Be sure your answer has the correct number of significant digits in it. I keep getting this problem wrong because of the sig. digits, dont round till the end because if it is off by 0.1, it will be incorrect.
Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of water formed from the reaction of 2.10g of ethane and 15.1g of oxygen gas? Be sure your answer has the correct number of significant digits in it. I keep getting this problem wrong because of the sig. digits, dont round till the end because if it is off by 0.1, it will be incorrect.
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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Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of water formed from the reaction of 2.10g of ethane and 15.1g of oxygen gas?
Be sure your answer has the correct number of significant digits in it.
I keep getting this problem wrong because of the sig. digits, dont round till the end because if it is off by 0.1, it will be incorrect.
![### Theoretical Yield of Water from Combustion of Ethane
#### Problem Statement:
Gaseous ethane \(\left( \text{CH}_3\text{CH}_3 \right)\) reacts with gaseous oxygen gas \(\left( \text{O}_2 \right)\) to produce gaseous carbon dioxide \(\left( \text{CO}_2 \right)\) and gaseous water \(\left( \text{H}_2\text{O} \right)\). What is the theoretical yield of water formed from the reaction of 2.10 g of ethane and 15.1 g of oxygen gas?
Be sure your answer has the correct number of significant digits in it.
#### Solution:
- **Input Box**: You will need to input your answer, expressed in grams of \(\text{H}_2\text{O}\).
#### Additional Controls:
- **Checkbox**: There's a checkbox option displaying \(\times 10\), which can be used for scientific notation.
- **Action Buttons**:
- **X**: Presumably a clear or delete button.
- **Reset Button**: To reset the values or calculation.
- **Help Button**: May provide hints or additional help for solving the problem.
#### Steps for Solution:
1. **Balance the chemical equation** for the combustion of ethane:
\[\text{C}_2\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O}\]
2. **Calculate the moles of ethane and oxygen** based on the given weights and their molar masses.
3. **Determine the limiting reagent to identify the theoretical yield** of water.
4. **Convert the moles of water produced to grams** using the molar mass of water.
Ensure that your final answer incorporates the correct number of significant digits as based on the initial data provided (2.10 g of ethane and 15.1 g of oxygen gas implies 3 and 4 significant digits, respectively).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8269917f-e65a-4c61-8f6b-ddb45740edf7%2Fcc0bd96f-fdb5-4c22-acb8-250556aab79c%2Fluxjmt_processed.png&w=3840&q=75)
Transcribed Image Text:### Theoretical Yield of Water from Combustion of Ethane
#### Problem Statement:
Gaseous ethane \(\left( \text{CH}_3\text{CH}_3 \right)\) reacts with gaseous oxygen gas \(\left( \text{O}_2 \right)\) to produce gaseous carbon dioxide \(\left( \text{CO}_2 \right)\) and gaseous water \(\left( \text{H}_2\text{O} \right)\). What is the theoretical yield of water formed from the reaction of 2.10 g of ethane and 15.1 g of oxygen gas?
Be sure your answer has the correct number of significant digits in it.
#### Solution:
- **Input Box**: You will need to input your answer, expressed in grams of \(\text{H}_2\text{O}\).
#### Additional Controls:
- **Checkbox**: There's a checkbox option displaying \(\times 10\), which can be used for scientific notation.
- **Action Buttons**:
- **X**: Presumably a clear or delete button.
- **Reset Button**: To reset the values or calculation.
- **Help Button**: May provide hints or additional help for solving the problem.
#### Steps for Solution:
1. **Balance the chemical equation** for the combustion of ethane:
\[\text{C}_2\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O}\]
2. **Calculate the moles of ethane and oxygen** based on the given weights and their molar masses.
3. **Determine the limiting reagent to identify the theoretical yield** of water.
4. **Convert the moles of water produced to grams** using the molar mass of water.
Ensure that your final answer incorporates the correct number of significant digits as based on the initial data provided (2.10 g of ethane and 15.1 g of oxygen gas implies 3 and 4 significant digits, respectively).
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