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At 1127 K and 1 atm pressure , a gaseous mixture of `CO and CO_(2)` in equilibrium with solid carbon has 90*55 % CO by mass in the reaction, `C(s) + CO_(2) (g) hArr 2 CO (g)`.
Calculate `k_(c) ` for the reaction at the above temperature.

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If total mass of the mixture of `CO and CO_(2)` is 100 g , then
` :. "At eqm., " [BrCl] = ( 3*30 xx 10^(-3) - 3*0 xx 10^(-3))= 0*30 xx 10^(-3) = 3*0 xx 10^(-4) "mol"L^(-1)`
Number of moles of ` :. "At eqm., " [BrCl] = ( 3*30 xx 10^(-3) - 3*0 xx 10^(-3))= 0*30 xx 10^(-3) = 3*0 xx 10^(-4) "mol"L^(-1)`
` :. p_(CO) = (3*234)/(3*234 + 0*215 ) xx 1" atm " = 0*938 " atm" , p_(CO_(2)) = (0*215)/(3*234 + 0*215 ) xx 1 "atm " = 0*062 "atm "`
` k_(p) = (p_(CO)^(2))/p_(CO_(2)) = (0*938 )^(2)/(0*062 )= 14 *19` .
` Delta n_(g) = 2-1 =1 :. K_(p) = K_(c) (RT) or K_(c) = (K_(p))/(RT) = (14*19)/(0*0821 xx 1127)=0*153 ` .

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