Question

For two reactions in equilibrium in same container
© A(s) = 2B(g) + C(g); (K), = 27 atm
( D(s) = 2B(9) + E(g); (Kn)2 = 81 atmº
Pressure of B(g) at equilibrium will be
(1) 6 atm
(2) 3 atm
(3) 5 atm
(4) 9 atm​

Answer 1

The Pressure of B(g) at equilibrium will be  3 atm.

Explanation:

First case:

A(s)  = 2B(g) + C (g)

Kp1 = 27 atm^3

Kp =(PB) ² (PC) /1  = 27

(PB) ²(PC) = 27 [ (PB) ²(PC) = 3^2 . 3]

Second case:

D(s)  ⇄ 2B (g) + E(g)

(KP)2 =  81 atm

(KP)^2 = (PB) ² (PE) / 1 = 81

(PB) ² . (PE)  = 3^2 x 9

On comparing the both cases it gives

(PB) = 3 atm

Thus the Pressure of B(g) at equilibrium will be  3 atm.

Also learn more

Calculate the pressure of a gas whose molar mass is 29.3 g mol , having density 1.29 kg at 273 K temperature.​?

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Answer 2

Answer: 6 atm

common ions get added hence it's 2x+2y for B.

hope it helps!