The reaction 2NO + Cl2 <==> 2NOCl has Kc= 210 what is the equilibrium concentration of NO in moles per liter given the following Cl2= .46 NOCl= .43M at equilibrium.
So far all ive gotten is
210= [.43]^2/[.46][NO]^2
where do I go from here please
The equation you have written can be solved for [NO]at equilibrium. Just use some algebra to rearrange it. You will need to take a square root of [NO]^2.
To solve for the equilibrium concentration of NO, we can rearrange the equation using the given values:
Kc = [NOCl]^2 / ([Cl2] * [NO]^2)
Rearranging the equation, we have:
[NO]^2 = ([Cl2] * [NOCl]^2) / Kc
Now, substitute the given values:
[NO]^2 = (.46 * (.43)^2) / 210
Simplify the expression:
[NO]^2 = 0.00042215476
Take the square root of both sides:
[NO] = √(0.00042215476)
[NO] ≈ 0.02054 M
Therefore, the equilibrium concentration of NO is approximately 0.02054 moles per liter.