A graduate student places 0 272 mol of PCl 3 (g) and 8 56 10 4 mol of PCl 5 (g) into a 0 718 L flask at a certain temperature PCl 5 (g) is known to dissociate as follows PCl 5 (g) PCl 3 (g) Cl 2 (g) After the reaction attains equilibrium, the student finds that the flask contains 2 51 10 4 mol of C...

PCl 5 g PCl 3 g Cl 2 g According to the given equation one mole of PCl ...

A graduate student places 0.272 mol of PCl 3 (g) and 8.56 10 -4 mol of

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A graduate student places 0.272 mol of PCl₃(g) and 8.56 × 10^-4 mol of PCl₅(g) into a 0.718-L flask at a certain temperature.

PCl₅(g) is known to dissociate as follows:

PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

After the reaction attains equilibrium, the student finds that the flask contains 2.51 × 10^-4 mol of Cl₂. Calculate the equilibrium constant K_c for the reaction at this temperature.

a. 0.114

b. 8.51 × 10²

c. 0.157

d. 8.88 × 10⁴

e. 2.40 × 10⁴

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General Chemistry

ISBN: 978-1439043998

9th edition

Authors: Darrell Ebbing, Steven D. Gammon

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Question Posted: Jun 14, 2020 08:02 AM

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A graduate student places 0.272 mol of PCl 3 (g) and 8.56 10 -4 mol of

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