# Gas Temperature and Pressure Relationship**Questions:**1. Based on the data collected in the table above, what trend can be observed for the temperature of a gas when the pressure of the gas is increased?2. Is this considered a direct or an indirect relationship between the variables?3. Press the reset button at the top right of the screen.**Using the temperature control arrows, reduce the temperature of the gas to 158K:**a. In the space below, record your observations regarding the behavior of the particles in the gas sample as the temperature is reduced. Be sure to discuss collisions in your comments.b. In the space below, calculate the new pressure value for the gas.c. Check your final answer for part b by clicking the calculate button next to P2.1. **a. Observations when Volume is reduced:** - **b. Calculation** \[ P1 = \frac{P2 \times T1}{T2} \]---# Practice Problems:1. Calculate the temperature of a gas when it is expanded to 5.25L. The gas originally occupies 3.45L of space at 282K.2. The temperature of a gas is increased from 125°C to 182°C inside a rigid container. The original pressure of the gas was 1.22 atm. What will the pressure of the gas be after the temperature change?3. The volume of gas in a container was originally 3.24L, while at standard pressure, 1.00 atm. What will the volume be if the pressure is increased to 1.20 atm?

1. Given that : The initial volume of the gas = 3.45 L The initial temperature of the gas = 282 K The final volume of the gas = 5.25 L We have to determine the final temperature of the gas.According to the Charles's law : V1T1=V2T2Here V1=initial volume and T1=initial temperatureV2=final volume and T2=final temperatureSo, putting known values, we get :3.45 L282 K=5.25 LT2So,T2=5.25 L×282 K3.45 L⇒429.13 K Thus, the temperature of the gas at 5.25 L volume is 429.13 K.2. Given that : The initial temperature of the gas = 125°C = (125 + 273) K= 398 K The initial pressure of the gas = 1.22 atm The final temperature of the gas = 182°C = (182 + 273) K = 455 K We have to determine the final pressure of the gas.According to the Gay-Lussac's law : P1T1=P2T2Here P1=initial pressure and T1=initial temperatureP2=final pressure and T2=final temperatureSo, putting known values, we get :1.22 atm398 K=P2455 KSo,P2=1.22 atm×455 K398 K⇒1.39 atm Thus, the pressure of the gas at 182°C temperature is 1.39 atm.3. Given that : The initial volume of the gas = 3.24 L The initial pressure of the gas = 1.00 atm The final pressure of the gas = 1.22 atm We have to determine the final volume of the gas.According to the Boyle's law : P1V1=P2V2Here P1=initial pressure and V1=initial volumeP2=final pressure and V2=final volumeSo, putting known values, we get :1.00 atm×3.24 L=1.22 atm×V2So,V2=1.00 atm×3.24 L1.22 atm⇒2.66 L Thus, the volume of the gas at 1.22 atm pressure is 2.66 L.

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1. Calculate the temperature of a gas when It is expanded to 5.25L. The gas originally occuples 3.45L of space at282K. 1. The temperature of a gas is increased from 125°C to 182°C inside of a rigid container. The original pressure of the gas was 1.22atm, what will the pressure of the gas be after the temperature change? 1. The volume of gas in a container was originally 3.24L, while at standard pressure, 1.00atm. What will the volume be if the pressure Is Increased to 1.20atm?

1. Calculate the temperature of a gas when It is expanded to 5.25L. The gas originally occuples 3.45L of space at282K. 1. The temperature of a gas is increased from 125°C to 182°C inside of a rigid container. The original pressure of the gas was 1.22atm, what will the pressure of the gas be after the temperature change? 1. The volume of gas in a container was originally 3.24L, while at standard pressure, 1.00atm. What will the volume be if the pressure Is Increased to 1.20atm?

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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