Consider the following equilibrium system: PCI5(9) PC13(g) + Cl₂(g) A 10.00 L evacuated flask is filled with 0.4163 mol PCIs(g) at 297.5 K. The temperature is then raised to 503.5 K, where the decomposition of PCIs gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 2.46E atm. What is the value of the equilbrium constant terms of concentrations, Kc, at 503.5 K? Kc =
Consider the following equilibrium system: PCI5(9) PC13(g) + Cl₂(g) A 10.00 L evacuated flask is filled with 0.4163 mol PCIs(g) at 297.5 K. The temperature is then raised to 503.5 K, where the decomposition of PCIs gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 2.46E atm. What is the value of the equilbrium constant terms of concentrations, Kc, at 503.5 K? Kc =
Chemistry
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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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Transcribed Image Text:Consider the following equilibrium system:
PCI5(9) PC13 (9) + Cl₂(g)
A 10.00 L evacuated flask filled with 0.4163 mol PCI5 (9) at 297.5 K. The temperature is then raised to 503.5 K, where the decomposition of PCIs gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask
atm.
What is the value of the equilbrium constant in terms of concentrations, Ko at 503.5 K?
Kc =
Transcribed Image Text:Consider the following equilibrium system:
PCI5(9) PC13 (9) + Cl₂(9)
A 10.00 L evacuated flask is filled with 0.4163 mol PCIs(g) at 297.5 K. The temperature is then raised to 503.5 K, where the decomposition of PCIs gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 2.468
atm.
What is the value of the equilbrium constant in terms concentrations, Kc, at 503.5 K?
Kc
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Here first we have to determine Kp then Kc using the relation between them.
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