At a certain temperature, the concentrations of NO and NH3 are equal, and the concentration of H2o and o2 are 2.0M and 3.0M respectively. What is the value of Keq at this temp? The equation is 5O2+4NH3--> 4NO+6H20
.......5O2 + 4NH3--> 4NO + 6H20
E........3M....x........x....2M
I assume that this is at equilibrium at this "certain" temperature. Also I assume the "certain" T is high enough that H2O is a gas. If all of that is so then NH3 must be 3M and H2O must be 2M
Plug in the numbers and calculate Keq.
Thanks so much! :)
To calculate the value of the equilibrium constant, Keq, at a certain temperature, we need to use the concentrations of the reactants and products at equilibrium. In this case, the given concentrations are:
[NO] = [NH3] (concentrations of NO and NH3 are equal)
[H2O] = 2.0 M
[O2] = 3.0 M
Based on the balanced equation:
5O2 + 4NH3 → 4NO + 6H2O
The expression for Keq can be written as:
Keq = ([NO]^4 * [H2O]^6) / ([O2]^5 * [NH3]^4)
Since [NO] = [NH3], we can substitute [NO] for [NH3] in the expression:
Keq = ([NO]^4 * [H2O]^6) / ([O2]^5 * [NO]^4)
Simplifying further:
Keq = [NO]^2 * [H2O]^6 / ([O2]^5)
Substituting the given values:
Keq = [NO]^2 * (2.0^6) / (3.0^5)
Now, since [NO] = [NH3], we can represent [NO] as x:
Keq = x^2 * 2.0^6 / 3.0^5
To solve for Keq, we need more information about the concentration of NO or NH3. Without that information, we cannot determine the exact value of Keq at this temperature.