For the given equilibrium reaction,2 A(g) rig | vedclass

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(B) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$.Here,$\Delta n = (2 + 1) - 2 = 1$.Given $T = 800 \ K

Vedclass · Accepted Answer

$0.026$

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(B) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$.Here,$\Delta n = (2 + 1) - 2 = 1$.Given $T = 800 \ K$ and $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$.Note: The value of $K_c$ changes with temperature. However,assuming the provided $K_c$ value is intended for the calculation at $800 \ K$ (as is common in such textbook problems),we use $K_c = 4 	imes 10^{-4}$.$K_p = (4 	imes 10^{-4}) 	imes (0.082 	imes 800)^1$.$K_p = 0.0004 	imes 65.6 = 0.02624 \approx 0.026$.

For the given equilibrium reaction,$2 A(g) \rightleftharpoons 2 B(g) + C(g)$,the equilibrium constant $(K_c)$ at $1000 \ K$ is $4 \times 10^{-4}$. Calculate $K_p$ for the reaction at $800 \ K$ temperature.

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