How many liters of gaseous hydrogen bromide at 55°C and 0.759 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid? L HBr
How many liters of gaseous hydrogen bromide at 55°C and 0.759 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid? L HBr
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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**Gas Law Application: Determining Gas Volume for Chemical Preparation**
**Question:**
How many liters of gaseous hydrogen bromide at 55°C and 0.759 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid?
**Instructions:**
- Enter your answer in the provided box.
- Box: [_________] L HBr
**Context for the Solution:**
To solve this problem, use the Ideal Gas Law and molarity concepts to calculate the volume of hydrogen bromide gas needed.
This involves:
1. Determining the moles of HBr required using the formula \( \text{Moles} = \text{Molarity} \times \text{Volume} \).
2. Applying the Ideal Gas Law: \( PV = nRT \), to find the necessary volume of gas.
Remember to convert the temperature to Kelvin by adding 273.15 to the Celsius temperature. Also, use the appropriate gas constant \( R \) in your calculations.
You have 3 attempts left to check your answer before your submission is finalized.
---
In the image, there are no graphs or diagrams visible, just a text box for entering the numerical answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F728e70e5-602c-40ad-8198-449db4e3e647%2F21e67597-4a13-4b3c-ae6e-c3466c0cb163%2Fcifvyz8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Sure, here is the transcription suitable for an educational website:
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**Gas Law Application: Determining Gas Volume for Chemical Preparation**
**Question:**
How many liters of gaseous hydrogen bromide at 55°C and 0.759 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid?
**Instructions:**
- Enter your answer in the provided box.
- Box: [_________] L HBr
**Context for the Solution:**
To solve this problem, use the Ideal Gas Law and molarity concepts to calculate the volume of hydrogen bromide gas needed.
This involves:
1. Determining the moles of HBr required using the formula \( \text{Moles} = \text{Molarity} \times \text{Volume} \).
2. Applying the Ideal Gas Law: \( PV = nRT \), to find the necessary volume of gas.
Remember to convert the temperature to Kelvin by adding 273.15 to the Celsius temperature. Also, use the appropriate gas constant \( R \) in your calculations.
You have 3 attempts left to check your answer before your submission is finalized.
---
In the image, there are no graphs or diagrams visible, just a text box for entering the numerical answer.
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