kingjewel1 Posted December 27, 2004 Posted December 27, 2004 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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