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Kp for H20g+C(s)<=>H2(g)+CO(g)

kingjewel1
in Chemistry

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at 1000K the equilibrium constant for

H20(g)+C(s)<=>H2(g)+CO(g)

is 3.72atm. If total pressure is 25atm what would the partial pressures be?

 

Could someone tell me if i've got the right answer in: 69% reacted.

therefore Partial pressures (Pg): Pg(H20)=3.875 Pg(H2)=8.625 Pg(CO)=8.625

 

i used x=reacted H20 1-x ; C 1 ; H2 x; CO x;

total=3

Xg= 1-x/2; unity; x/2; x/2; for the compounds respectively.

i'm not sure how to treat carbon as it is solid. do i count it as 1 when calculating the equilibrium total moles?

 

thanks in advance.

my Alevel is in a week n i'm not sure of this one

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