The equilibrium constant of the dissociation reaction H2 ?

Chapter 16, Problem 7P

(choose chapter or problem)

The equilibrium constant of the dissociation reaction \(\mathrm{H}_{2} \rightarrow 2 \mathrm{H}\) at \(3000 \mathrm{~K}\) and \(1 \mathrm{~atm}\) is \(K_{P}\). Express the equilibrium constants of the following reactions at \(3000 \mathrm{~K}\)in terms of \(K_{P_{1}}\) :

(a) \(\mathrm{H}_{2} \rightleftharpoons 2 \mathrm{H}\)

at \(2 \mathrm{~atm}\)

(b) \(\quad 2 \mathrm{H} \rightleftharpoons \mathrm{H}_{2}\)

at \(1 \mathrm{~atm}\)

(c) \(\quad 2 \mathrm{H}_{2} \rightleftharpoons 4 \mathrm{H}\)

(d) \(\mathrm{H}_{2}+2 \mathrm{~N}_{2} \rightleftharpoons 2 \mathrm{H}+2 \mathrm{~N}_{2} \quad\) at \(2 \mathrm{~atm}\)

(e) \(\quad 6 \mathrm{H} \rightleftharpoons 3 \mathrm{H}_{2} \quad\)at \(4 \mathrm{~atm}\)

Equation Transcription:

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Text Transcription:

H_2 rightarrow 2H

s

3000 K

1  atm

K_P_1

3000 K

K_P_1

H_2 leftrightharpoons 2H     2 atm

2H leftrightharpoons H_2    1 atm

2H_2 leftrightharpoon 4H   1 atm

H_2+2N_2 leftrightharpoons 2H+2N_2   2 atm

6H leftrightharpoons 3H_2    4 atm