At 527 ^oC,the reaction given below has K_c | vedclass

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(C) Given reaction: $NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$ with $K_{c1} = 4$.For the target reaction: $N_{2(g)} +

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$\left( \frac{1}{4 	imes 800R} ight)^2$

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(C) Given reaction: $NH_{3(g)} ightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$ with $K_{c1} = 4$.For the target reaction: $N_{2(g)} + 3H_{2(g)} ightleftharpoons 2NH_{3(g)}$,we reverse the first reaction and multiply by $2$.Thus,$K_{c2} = (1/K_{c1})^2 = (1/4)^2 = 1/16$.The relationship between $K_P$ and $K_c$ is $K_P = K_c(RT)^{\Delta n}$.For the target reaction,$\Delta n = 2 - (1 + 3) = -2$.Temperature $T = 527 + 273 = 800 \ K$.$K_P = (1/16) 	imes (R 	imes 800)^{-2} = (1/4)^2 	imes (800R)^{-2} = \left( \frac{1}{4 	imes 800R} ight)^2$.

At $527 \ ^oC$,the reaction given below has $K_c = 4$.
$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$
What is the $K_P$ for the following reaction?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

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At $527 \ ^oC$,the reaction given below has $K_c = 4$.$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$What is the $K_P$ for the following reaction?$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$