The two common chlorides of Phosphorus, PCl3 and PCl5, both important in the production of other phosphorous compounds, coexist in equilibrium as shown in the balanced chemical reaction below:
PCl3 (g) + Cl2 (g) <-----> PCl5 (g)

At 250 C, an equilibrium mixture in a 2.50 L flask contains 0.305 g PCl5, 0.440 g PCl3, and 4.24 g Cl2.

A. Show the equilibrium Constant formula.

B. What is the value of Kc for this reaction? Hint: Use molarity in the Kc calculations.

A.
Kc = [PCl5]/([Cl2][PCl3])
B.
1.826

1. 👍 0
2. 👎 0
3. 👁 1,285
1. A is OK.
I don't get that for B
What concns do you have for each?

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2. 👎 0
2. I got 0.23887323 for Cl2, 0.001281584 for PCl3, and 0.000586862 for PCl5.

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2. 👎 0
3. Check that Cl2. 4.24/70.9.2.5 = 0.0239

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2. 👎 0

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