Chemistry | VITEEE 2019 | Discussion Page

The value of K_C for the reaction: A+3B $\rightleftharpoons$ 2C at 400ºC is 0.5.Calculate the value of K_P

$1.6\times 10^{-4}$

$1.6\times 10^{-6}$

$1.6\times 10^{-5}$

$1.6\times 10^{-3}$

Option A

K_P = K_C [RT]^Δng Δn = 2-4 = -2

T = 673K, K_C = 0.5,

R=0.082L.atm.mol^-1 K^-1

K_P= 0.5×[0.082×673]^-2

= $1.6\times 10^{-4}$

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