find the equilibrium concentrations of all the species in the following reaction

Question

find the equilibrium concentrations of all the species in the following reaction.

2H2S(g) = 2H2(g) +S2(g) Kc = 1.67x10-7 @ 800C

that starting concentrations of H2S and S2 = .0400M and H2=.0800 M

i have the ice tables set up with and get Kc = ((.0800+2x)^2 (.0400+x))/(.04-2x)^2

when i solve analyticaly for x i get x=-.03916 and when i cross out the 2x in both of the squared equations i get .0399999

both of which imply i can assume the product goes entirely back to H2S. but what would be the correct way of solving the problem when you dont have anything more than a basic calculator.

Explanation / Answer

From the solutions of quadratic equations, it is better to select a solution which is a positive number and least value than the initial concentration as a change

Hence, Among the solutions -

x = 0.03999 is correct to take as a change.

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