Using the equilibrium constant expression given below,=KeqNH32N2H23and the equilibrium constant, =Keq0.575, determine the equilibrium concentration of NH3 if the concentration of N2 is ×4.310−2M, and the concentration of H2 is ×6.810−3M. Round your answer to 2 significant figures.
Question
Using the equilibrium constant expression given below,=KeqNH32N2H23and the equilibrium constant, =Keq0.575, determine the equilibrium concentration of NH3 if the concentration of N2 is ×4.310−2M, and the concentration of H2 is ×6.810−3M. Round your answer to 2 significant figures.
Solution
The equilibrium constant expression is given by:
Keq = [NH3]^2 / ([N2] * [H2]^3)
We know that Keq = 0.575, [N2] = 4.31 x 10^-2 M, and [H2] = 6.81 x 10^-3 M. We need to find [NH3].
Let's rearrange the equation to solve for [NH3]:
[NH3] = sqrt(Keq * [N2] * [H2]^3)
Substitute the given values into the equation:
[NH3] = sqrt(0.575 * 4.31 x 10^-2 M * (6.81 x 10^-3 M)^3)
Calculate the value inside the square root first:
= sqrt(0.575 * 4.31 x 10^-2 M * 3.16 x 10^-7 M^3)
= sqrt(7.8 x 10^-4)
Finally, take the square root:
[NH3] = 0.028 M
So, the equilibrium concentration of NH3 is 0.028 M, rounded to two significant figures.
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