I do not understand this topic at all. I keep thinking I’m doing it right but I’m wrong each time. Will you please help me and write out the steps.
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Consider the following system at equilibrium where AH° = -198 k], and Kc = 34.5 , at 1.15><103 K: 2 502 (g) + 02 (g) H 2 803 (g) Ifthe TEMPERATURE on the equilibrium system is suddenly increased : The value of Kc II A. Increases B. DecreasesC. Remains the same The value of Qc D A. Is greater than Kc B. Is equal to KcC. Is less than Kc The reaction must: I:I A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium.C. Remain the same. Already at equilibrium. The concentration of 02 will: D A. Increase. B. Decrease.C. Remain the same.