What Is the Equilibrium Concentration of CO in the Reaction at 400K?

[ada15]

Homework Statement

CO(g) + NH_3(g) ...> HCONH_2(g)

euilibrium constant is: K = 0.207 at 400 K
If a reaction is filled with intial concentrations 2.20 M of CO and 2.60 M of NH_3 and the reactanats are allowed to raect at 400K/ what will be the concentrations of CO at equilibrium ?

Homework Equations

Keq = [HCONH_2] / [CO] [NH_3]

The Attempt at a Solution

0.207 = (X) /(2.20-X)(2.6-X)

But I'm getting the wrong answer for x. Please help me.

 

[qwedsa]

^your equation for x seems correct. i rearranged it to
0 = 5.72/x - 5.007 + x
we need to find the zeroes

when graphed, the zeros are 1.76 and 3.24

if we use 3.24, we would have a negative concentration of both CO and NH3, which is physically impossible. so, we go with 1.76

so the answer: 2.2 M - 1.76 = 0.44 M

 

[Blueshift5]

I would approach this problem by first understanding the concept of equilibrium concentration. Equilibrium concentration refers to the concentrations of reactants and products that exist at equilibrium, when the rate of the forward reaction is equal to the rate of the reverse reaction. In other words, it is the point at which the concentrations of reactants and products no longer change.

To find the equilibrium concentration of CO in this reaction, we can use the equilibrium constant equation you provided: Keq = [HCONH_2] / [CO][NH_3]. Since we are given the value of Keq (0.207) and the initial concentrations of CO (2.20 M) and NH_3 (2.60 M), we can rearrange the equation to solve for the equilibrium concentration of CO:

[CO] = [HCONH_2] / (Keq * [NH_3])

Substituting the given values, we get:

[CO] = (0.207) / (2.60 * 2.20) = 0.036 M

Therefore, at equilibrium, the concentration of CO will be 0.036 M. It is important to note that this calculation assumes that the reaction has reached equilibrium and that the concentrations of all other species remain constant. If the reaction has not yet reached equilibrium, the concentrations of reactants and products will continue to change until equilibrium is reached.