Question
In: Chemistry
Consider the reaction CO(g)+NH3(g)⇌HCONH2(g), Kc=0.760 If a reaction vessel initially contains only CO and NH3 at concentrations...
Consider the reaction
CO(g)+NH3(g)⇌HCONH2(g), Kc=0.760
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?
Solutions
Expert Solution
The reaction is :
CO(g) + NH3(g) ⇌ HCONH2(g),
Initial 1 2 0
Change -x -x +x
Equilbrium 1-x 2-x x
Kc = [ HCONH2] / [CO2] [ NH3] = 0.760
0.760 = x / (1-x)(2-x)
0.760 = x / 2 -x -2x +x^2
1.52 - 2.28x + 0.760x^2 = x
0.760x^2 - 3.28x +1.52 = 0
on solving
x = 0.528M
Therefore equilibrium concentrations will be
[CO2] = 1 - 0.528 = 0.472 M
[NH3] = 2 - 0.528 = 1.472 M
[ HCONH2] = 0.528M
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