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Consider the following reaction: 2AB(g) <--> A2(g) + B2(g) 4.25 moles of AB are placed in a 1.00 L flask and the system is allowed to come to -quilibrium, at which time 64.3% of AB remained. Calculate Kc.

Consider the following reaction: 2AB(g) <--> A2(g) + B2(g) 4.25 moles of AB are placed in a 1.00 L flask and the system is allowed to come to -quilibrium, at which time 64.3% of AB remained. Calculate Kc.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
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Consider the following reaction: 2AB(g) <--> A2(g) + B2(g) 4.25 moles of AB are placed in a 1.00 L flask and the system is allowed to come to equilibrium, at which time 64.3% of AB remained. Calculate K..
Transcribed Image Text:Consider the following reaction: 2AB(g) <--> A2(g) + B2(g) 4.25 moles of AB are placed in a 1.00 L flask and the system is allowed to come to equilibrium, at which time 64.3% of AB remained. Calculate K..
Expert Solution
Step 1

Given equilibrium reaction is:

2AB(g)  ⇌  A2(g)+B2(g)

Initial amount of AB is 4.25mol. in 1.00L flask.

At equilibrium 64.3% of AB remained.

Calculate Kc.

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