A reaction mixture at equilibrium at 175 k contains ph2 = 0.958 atm, pi2 = 0.877 atm, and phi = 0.020 atm. a second reaction mixture, also at 175 k, contains ph2 = pi2 = 0.621 atm, and phi = 0.101 atm. is the second reaction at equilibrium? if not, what will be the partial pressure of hi when the reaction reaches equilibrium at 175 k?

Question

Chemistry

Trace Salas

25 August, 00:14

A reaction mixture at equilibrium at 175 k contains ph2 = 0.958 atm, pi2 = 0.877 atm, and phi = 0.020 atm. a second reaction mixture, also at 175 k, contains ph2 = pi2 = 0.621 atm, and phi = 0.101 atm. is the second reaction at equilibrium? if not, what will be the partial pressure of hi when the reaction reaches equilibrium at 175 k?

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Answers (1)

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Juliet Short · Answer 1

from ICE table

H2 (g) + I2 (g) ↔ 2HI (g)

equ 0.958 0.877 0.02 first mix1

0.621 0.621 0.101 sec mix2

Kp1 = P (HI) ^2 / p (H2) * p (I2) for mix 1

= 0.02^2 / 0.958*0.877

= 4.8x10^-4

Kp2 = P (HI) ^2 / P (H2) * P (I2) for mix 2

= 0.101^2 / 0.621*0.621

= 0.0265

we can see that Kp1< Kp2 that means that the sec mixture is not at equilibrium. It will go left to reduce its products and increase reactant to reduce the Kp value to achieve equilibrium.

and the partial pressure of Hi when mix 2 reach equilibrium is:

4.8x10^-4 = P (Hi) ^2 / (0.621*0.621)

∴ P (Hi) at equilibrium = 0.0136 atm