marks People Window Help 4) 82%(.) Wed Mar 14 5:13 PM Consic Welc0 m/ilrn/t ple

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marks People Window Help 4) 82%(.) Wed Mar 14 5:13 PM Consic Welc0 m/ilrn/t ple v Yahoo! .. YouTubewkipedia News / WebAssign Esader D.MyEPCC tivity.do?locator assignment-take&takeAssignmentSessionLocator-assignment-take; Consider the following system at equilibrium where H.-10.4 k, and Ke-130×10' at 698 K: 2HI(g)H2()+ 12(8) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of KA. Increases B. Decreases C. Remains the same The value of eA. Is greater than K B. Is equal to K C. Is less than K The reaction must: 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 Iz will: A Increase. B. Decrease. C. Remain the same. Submilt Answer Retry Entre Group 9 more group attempts remaining 400 level in General MacBook Pro 4) F8

Explanation / Answer

Since Delta H is positive, it is endothermic reaction and occurs at high temperature.

With the decrease of temperature, Kc decreases.

Since forward reaction is endothermic occurs at high temperature, A/C to Le Charlier's principle , the reaction goes back on decreasing temperature.

Qc > Kc, since Q= [H2][I2]/[HI]2 = 1.1/12 =1 > 1.8x10*-8

Reaction moles in reverse direction since Qc>Kc

Concentration of I2 will decreases.

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