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Hydrogen is manufactured on an industrial scale by this sequence of reactions: Write an equation that gives the overall equilibrium constant in terms of the equilibrium constants and . If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator.

User Seyit
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The question is incomplete. The complete question is :

Hydrogen is manufactured on an industrial scale by this sequence of reactions:


$CH_3(g) + H_2O(g) \rightleftharpoons CO(g) + 3H_2(g ) \ \ \ \ \ \ \ \ \ \ K_1$


$CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g) \ \ \ \ \ \ \ \ \ \ \ \ K_2$

The net reaction is :


$CH_4(g) + 2H_2O(g) \rightleftharpoons CO_2(g) + 4H_2(g) \ \ \ \ \ \ \ \ \ K$

Write an equation that gives the overall equilibrium constant
K in terms of the equilibrium constants
K_1 and
K_2. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator.

Solution :


$CH_3(g) + H_2O(g) \rightleftharpoons CO(g) + 3H_2(g ) \ \ \ \ \ \ \ \ \ \ K_1$


$K_1 = ([CO][H_2]^3)/([CH_4][H_2O])$ ...............(1)


$CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g) \ \ \ \ \ \ \ \ \ \ \ \ K_2$


$K_2 = ([CO_2][H_2])/([CO][H_2O])$ ...................(2)


$CH_4(g) + 2H_2O(g) \rightleftharpoons CO_2(g) + 4H_2(g) \ \ \ \ \ \ \ \ \ K$


$K=([CO_2][H_2]^4)/([CH_4][H_2O]^2)$

On multiplication of equation (1) and (2), we get


$K_1 * K_2=([CO][H_2]^3)/([CH_4][H_2O]) * ([CO_2][H_2])/([CO][H_2O])$


$K_1K_2=([CO_2][H_2]^4)/([CH_4][H_2O]^2)$ .................(4)

Comparing equation (3) and equation (4), we get


$K=K_1K_2$

User Eldshe
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