Consider the reaction, which takes place at a certain elevated temperature CO(g)+NH3(g)⇌HCONH2(g), Kc=0.710 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?

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Alleei Alleei · Answer 1 · 2020-03-12T09:20:14+01:00

Answer : The concentration of [tex]HCONH_2[/tex] at equilibrium is, 0.513 M

Explanation :

The given chemical reaction is:

[tex]CO(g)+NH_3(g)\rightleftharpoons HCONH_2(g)[/tex]

Initial conc. 1.00 2.00 0

At eqm. (1.00-x) (2.00-x) x

The expression for equilibrium constant is:

[tex]K_c=\frac{[HCONH_2]}{[CO][NH_3]}[/tex]

Now put all the given values in this expression, we get:

[tex]0.710=\frac{(x)}{(1.00-x)\times (2.00-x)}[/tex]

x = 0.513 and x = 3.89

We are neglecting value of x = 3.89 because equilibrium concentration can not be more than initial concentration.

Thus, the value of x will be, 0.513

The concentration of [tex]HCONH_2[/tex] at equilibrium is, 0.513 M