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A large balloon is initially filled with 1.00 mole of gas which has a volume of 22.0 L at 273 K and a pressure of 1.00 atm, what is the experimental ideal gas constant at this condition?

A large balloon is initially filled with 1.00 mole of gas which has a volume of 22.0 L at 273 K and a pressure of 1.00 atm, what is the experimental ideal gas constant at this condition?

Chemistry
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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**Question:** A large balloon is initially filled with 1.00 mole of gas which has a volume of 22.0 L at 273 K and a pressure of 1.00 atm. What is the experimental ideal gas constant at this condition? **Explanation:** To determine the experimental ideal gas constant \( R \) under the given conditions, we can use the Ideal Gas Law, which is expressed as: \[ PV = nRT \] In this equation: - \( P \) is the pressure, - \( V \) is the volume, - \( n \) is the number of moles, - \( R \) is the ideal gas constant, - \( T \) is the temperature in Kelvin. Given: - \( P = 1.00 \) atm, - \( V = 22.0 \) L, - \( n = 1.00 \) mole, - \( T = 273 \) K. Rearranging the Ideal Gas Law to solve for \( R \): \[ R = \frac{PV}{nT} \] Substituting the given values: \[ R = \frac{(1.00 \, \text{atm}) \times (22.0 \, \text{L})}{(1.00 \, \text{mol}) \times (273 \, \text{K})} \] Calculate \( R \) to find the experimental ideal gas constant.
Transcribed Image Text:**Question:** A large balloon is initially filled with 1.00 mole of gas which has a volume of 22.0 L at 273 K and a pressure of 1.00 atm. What is the experimental ideal gas constant at this condition? **Explanation:** To determine the experimental ideal gas constant \( R \) under the given conditions, we can use the Ideal Gas Law, which is expressed as: \[ PV = nRT \] In this equation: - \( P \) is the pressure, - \( V \) is the volume, - \( n \) is the number of moles, - \( R \) is the ideal gas constant, - \( T \) is the temperature in Kelvin. Given: - \( P = 1.00 \) atm, - \( V = 22.0 \) L, - \( n = 1.00 \) mole, - \( T = 273 \) K. Rearranging the Ideal Gas Law to solve for \( R \): \[ R = \frac{PV}{nT} \] Substituting the given values: \[ R = \frac{(1.00 \, \text{atm}) \times (22.0 \, \text{L})}{(1.00 \, \text{mol}) \times (273 \, \text{K})} \] Calculate \( R \) to find the experimental ideal gas constant.
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