Calculate for the temperature of 20.0 moles of argon that is kept in a 10.0 liter cylinder at a pressure of 150 atmospheres using the van der Waals equation. Compare the answer with the temperature that you would get if you would have solved for the temperature using the ideal gas equation (van der Waals constants for argon: a = 1.34 L² atm mol?, b = 0.0322 L mol")
Calculate for the temperature of 20.0 moles of argon that is kept in a 10.0 liter cylinder at a pressure of 150 atmospheres using the van der Waals equation. Compare the answer with the temperature that you would get if you would have solved for the temperature using the ideal gas equation (van der Waals constants for argon: a = 1.34 L² atm mol?, b = 0.0322 L mol")
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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Please answer only number 2
Handwritten or computerized solution is accepted as long it is readable and detailed.
Transcribed Image Text:IV. Calculations (5 pts. each)
Direction: Answer the problems below and make sure to show your solutions.
1. Calculate for the temperature of 20.0 moles of argon that is kept in a 10.0 liter
cylinder at a pressure of 150 atmospheres using the van der Waals equation.
Compare the answer with the temperature that you would get if you would have
solved for the temperature using the ideal gas equation (van der Waals constants
for argon: a = 1.34 L² atm mol?, b = 0.0322 L mol")
2. A food product has a water activity of 0.15 at a temperature of 10°C. At room
temperature (25°C), the water activity has been measured to be at 0.42. Calculate
for the heat of sorption (Q) in the transition from 10°C to 25°C (value for R is 8.314
JK' mol")
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