K c = 255 @1000 K for the given reaction:CO (g) + Cl 2 (g) <---> COCl 2(g) A rea
ID: 691174 • Letter: K
Question
Kc = 255 @1000 K for the given reaction:CO(g) + Cl2 (g) <---> COCl2(g) A reaction mixture initally contains a CO concentration of0.1450 M and a Cl2 concentration of 0.179 M at 1000K. 1) What is the equilibrium concentration of CO @ 1000 K? 2) What is the equilibrium concentration of Cl2 @1000K? 3) What is the equilibrium concentration of COCl2 @1000K? Kc = 255 @1000 K for the given reaction:CO(g) + Cl2 (g) <---> COCl2(g) A reaction mixture initally contains a CO concentration of0.1450 M and a Cl2 concentration of 0.179 M at 1000K. 1) What is the equilibrium concentration of CO @ 1000 K? 2) What is the equilibrium concentration of Cl2 @1000K? 3) What is the equilibrium concentration of COCl2 @1000K? A reaction mixture initally contains a CO concentration of0.1450 M and a Cl2 concentration of 0.179 M at 1000K. 1) What is the equilibrium concentration of CO @ 1000 K? 2) What is the equilibrium concentration of Cl2 @1000K? 3) What is the equilibrium concentration of COCl2 @1000K?Explanation / Answer
let x be the concentration of COCl2 formed atEquilibrium CO(g) + Cl2 (g) <---> COCl2(g) initialconc. 0.145 0.179 0 change -x -x x Equbconc. 0.145-x 0.179-x x Given Equilibrium constant , Kc = 255 By the definition of Kc , Equilibrium constant , Kc = [COCl2 ] / ( [CO] [ Cl2] ) 255 = x / ( ( 0.145-x ) * ( 0.179 - x ) ==> x^2 - 0.3279 x + 0.0259 = 0 x = { -(-0.3279 )±[( -0.3279)^2 - 4 ( 1 ) ( 0.0259 ) ] } / 2(1) =[0.3279 ± 0.039 ] / 2 =(0.3279 ± 0.0624 ) / 2 x = 0.1951M (omit since it is higher hanthe initial conc. of CO ) or x =0.1127 M So [COCl2 ] = 0.1127 M [CO] = 0.145-x = 0.145 - 0.1127 = 0.0323 M [Cl2 ] = 0.179-0.1127 = 0.0663 MRelated Questions
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