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The standard Gibbs energy change at 300 K for the reaction `2 A hArr B+ C " is" 2494 *2 J` At a given time, the composition of the reaction mixture is `[A] =1/2 , [B] =2 and [C] =1/2 .` The reaction proceeds in the : `[R=8*314 J//K//mol, e=2*718]`A. Forward direction because `Q gt K_(c)`B. Reverse direction because `Q gt K_(c)`C. Forward direction because `Q lt K_(c)`D. Reverse direction because `Q lt K_(c)` |
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Answer» Correct Answer - B `Delta G^(@) = -2*30" RT "log K_(c)` ` 2494.2 = - 2*303 (8.314) (300) log K_(c)` or log `K_(c) =-0*4342` or `K_(c)= "antilog" (bar 1*5658) = 0*3679` Now , when `[A] =1/2, [B] = 2 and [C] = 1/2` `Q_(c)= ([B][C])/([A]^(2)) = (2xx1/2)/((1/2)^(2))=4` As `Q_(c) gt K_(c),` reaction will proceed in the reverse direction. |
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