c. Calculate the mole fraction of chlorine and its partial pressure in the mixture of gases produced. d. The van der Waals equation applies strictly to pure real gases. P = (nRT/ V-nb) – a(n2/V2) Suppose the gas mixture generated in the decomposition has the following parameters: a= 4.00 atm*L2/mol2 and b = 0.0330 L/mol. Determine the pressure of the gas mixture in part (b) using the van der Waals equation. Why is the result smaller than that in part (b)?
c. Calculate the mole fraction of chlorine and its partial pressure in the mixture of gases produced. d. The van der Waals equation applies strictly to pure real gases. P = (nRT/ V-nb) – a(n2/V2) Suppose the gas mixture generated in the decomposition has the following parameters: a= 4.00 atm*L2/mol2 and b = 0.0330 L/mol. Determine the pressure of the gas mixture in part (b) using the van der Waals equation. Why is the result smaller than that in part (b)?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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c. Calculate the mole fraction of chlorine and its partial pressure in the mixture of gases produced.
d. The van der Waals equation applies strictly to pure real gases.
P = (nRT/ V-nb) – a(n2/V2)
Suppose the gas mixture generated in the decomposition has the following parameters: a= 4.00 atm*L2/mol2 and b = 0.0330 L/mol. Determine the pressure of the gas mixture in part (b) using the van der Waals equation. Why is the result smaller than that in part (b)?
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Step 1: Formulate Mole fraction and partial pressure
VIEWStep 2: Calculate mole fraction and parrtial pressure of chlorine gas
VIEWStep 3: Calculate total pressure of gas mixture according to real gas equation
VIEWStep 4: Explain the discrepancy of calculated pressure value according to real gas, form ideal gas
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