If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium? Kc=0.880
If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium? Kc=0.880
CO + NH3 = HCONH2
this is already balanced
Kc = [HCONH2 ] /([CO][NH3])
initially
[HCONH2 ] = 0
[CO] = 1
[NH3] = 2
in equilbirium
[HCONH2 ] = 0 + x
[CO] = 1 - x
[NH3] = 2 - x
substitute in K
K = 0.88
0.88 = (0 + x) /((1-x)(2-x))
0.88 (2 -3x + x ^2) = x
2 -3x + x ^2 = 1.136x
x^2 - (4.136)x +2 = 0
x = 0.5591
[HCONH2 ] = 0 + x = 0.5591
[CO] = 1 - x = 1-0.5591 = 0.4409
[NH3] = 2 - x = 1.4409
[HCONH2 ] = 0 + x = 0.5591
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