How many moles of air are there in a 2.0 L bottle at 19°C and 747 mm Hg? • PV=nRT • R = 0.0821 (L atm) (mol K) • R = 62.4 (L mm Hg) (K mol) • R = 8.31 (L kPa) (K mol)
How many moles of air are there in a 2.0 L bottle at 19°C and 747 mm Hg? • PV=nRT • R = 0.0821 (L atm) (mol K) • R = 62.4 (L mm Hg) (K mol) • R = 8.31 (L kPa) (K mol)
Human Anatomy & Physiology (11th Edition)
11th Edition
ISBN:9780134580999
Author:Elaine N. Marieb, Katja N. Hoehn
Publisher:Elaine N. Marieb, Katja N. Hoehn
Chapter1: The Human Body: An Orientation
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![**Understanding the Calculation of Moles of Air in a Given Volume**
When calculating the number of moles of air in a 2.0 L bottle at 19°C and 747 mm Hg, we use the Ideal Gas Law, which is represented by the formula:
**PV = nRT**
**Where:**
- **P** is the pressure of the gas.
- **V** is the volume of the gas.
- **n** is the number of moles of gas.
- **R** is the ideal gas constant.
- **T** is the temperature in Kelvin.
**Given Values:**
- Volume (V) = 2.0 liters
- Temperature (T) = 19°C = 19 + 273 = 292 K (conversion from Celsius to Kelvin)
- Pressure (P) = 747 mm Hg
**Values for the Ideal Gas Constant (R):**
1. **R = 0.0821 (L atm) / (mol K)**
2. **R = 62.4 (L mm Hg) / (K mol)**
3. **R = 8.31 (L kPa) / (K mol)**
In this scenario, since the pressure is given in mm Hg, we'll use the second value for R:
**R = 62.4 (L mm Hg) / (K mol)**
Using these variables in the ideal gas law formula, we can solve for the number of moles (n) of air in the bottle.
This educational example illustrates how to apply the Ideal Gas Law to find the quantity of moles in a given volume of gas under specific conditions of temperature and pressure.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6746fa6f-1856-443b-addc-ecae5d9da9b9%2Fd81c328f-8d0a-4eeb-a921-deee46457aa1%2Foxzxy0j_processed.png&w=3840&q=75)
Transcribed Image Text:**Understanding the Calculation of Moles of Air in a Given Volume**
When calculating the number of moles of air in a 2.0 L bottle at 19°C and 747 mm Hg, we use the Ideal Gas Law, which is represented by the formula:
**PV = nRT**
**Where:**
- **P** is the pressure of the gas.
- **V** is the volume of the gas.
- **n** is the number of moles of gas.
- **R** is the ideal gas constant.
- **T** is the temperature in Kelvin.
**Given Values:**
- Volume (V) = 2.0 liters
- Temperature (T) = 19°C = 19 + 273 = 292 K (conversion from Celsius to Kelvin)
- Pressure (P) = 747 mm Hg
**Values for the Ideal Gas Constant (R):**
1. **R = 0.0821 (L atm) / (mol K)**
2. **R = 62.4 (L mm Hg) / (K mol)**
3. **R = 8.31 (L kPa) / (K mol)**
In this scenario, since the pressure is given in mm Hg, we'll use the second value for R:
**R = 62.4 (L mm Hg) / (K mol)**
Using these variables in the ideal gas law formula, we can solve for the number of moles (n) of air in the bottle.
This educational example illustrates how to apply the Ideal Gas Law to find the quantity of moles in a given volume of gas under specific conditions of temperature and pressure.
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