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b. The equilibrium constant for the reaction 2H2(g) + S2(g) 2H2S(g) is Keq = . (3 points)

i. If a sample at equilibrium contained 0.051 M H2, 0.087 M S2, and 0.97 M H2S, what would Keq be for this reaction at that temperature? (2 points)


ii. What would happen to the equilibrium conditions if more S2 were added to the system? (1 point)

Respuesta :

sebassandin

Answer:

i. Keq=4157.99.

ii. More hydrogen sulfide will be produced.

Explanation:

Hello,

i. In this case, for the concentrations at equilibrium on the given chemical reaction, the equilibrium constant results:

[tex]Keq=\frac{[H_2S]^2}{[H_2]^2[S_2]} =\frac{(0.97M)^2}{(0.051M)^2(0.087)} =4157.99[/tex]

ii. Now, by means of the Le Chatelier's principle, the addition of a reactant shifts the reaction towards products, it means that more hydrogen sulfide will be produced in order to reach equilibrium.

Best regards.

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