At 450oC the value of equilibrium constant for the following system is 6.59 x 10-3. If [NH3] = 1.23 x 10-4 and [H2] = 2.75 x 10-3 at equilibrium, determine the concentration of N2 at that point.
N2(g) + 3H2(g) 2NH3(g)
Do you mean at equilibrium (NH3) = 1.23E-4M?
and (H2) at equilibrium = 2.75E-3M?
that is, is that M?
........N2 + 3H2 ==> 2NH3
E.......x....2.75E-3....1.23E-4M
Keq = (NH3)^2/(x)(H2)^3
Substitute and solve for x
To find the concentration of N2 at equilibrium, we can use the equation for the equilibrium constant, Kc:
Kc = [NH3]^2 / ([N2] * [H2]^3)
Given:
Kc = 6.59 x 10^-3
[NH3] = 1.23 x 10^-4
[H2] = 2.75 x 10^-3
We need to find [N2].
First, substitute the given values into the equation:
6.59 x 10^-3 = (1.23 x 10^-4)^2 / ([N2] * (2.75 x 10^-3)^3)
Simplify:
6.59 x 10^-3 = (1.5129 x 10^-8) / ([N2] * 2.4600625 x 10^-9)
Multiply both sides by [N2] * 2.4600625 x 10^-9:
6.59 x 10^-3 * [N2] * 2.4600625 x 10^-9 = 1.5129 x 10^-8
Multiply the numbers:
[ N2 ] * 1.61521324625 x 10^-11 = 1.5129 x 10^-8
Divide both sides by 1.61521324625 x 10^-11:
[ N2 ] = (1.5129 x 10^-8) / (1.61521324625 x 10^-11)
[N2] is approximately 9.365 x 10^2 or 936.5. Therefore, the concentration of N2 at equilibrium is 936.5.
To determine the concentration of N2 at equilibrium, we need to use the equilibrium constant expression for the given reaction:
Kc = [NH3]^2 / ([N2] × [H2]^3)
Given:
Kc = 6.59 × 10^(-3)
[NH3] = 1.23 × 10^(-4)
[H2] = 2.75 × 10^(-3)
We need to rearrange the equilibrium constant expression to solve for [N2]:
[N2] = [NH3]^2 / (Kc × [H2]^3)
Now let's substitute the given values into the equation:
[N2] = (1.23 × 10^(-4))^2 / (6.59 × 10^(-3) × (2.75 × 10^(-3))^3)
Simplifying the equation:
[N2] = 1.513 × 10^(-8) / (2.75 × 10^(-3))^3
[N2] = 1.513 × 10^(-8) / 2.39 × 10^(-11)
[N2] ≈ 632.3
Therefore, the concentration of N2 at equilibrium is approximately 632.3.