Consider the decomposition of a metal oxide to its elements where m represents a generic metal.
M2O(s)<->2M(s)+1/2O2(g)
the delta G is 10.30
I need to find K and PressureO2 at 298K I know the equations but i keep getting the answer wrong could you please help me. Could you show me all of the work.
It's much easier for you to show your work and let us critique it.
I had to calculate delta G which came out to be 10.30 then i had to solve for Kp so I used the equation
DeltaG=-RT(ln Kp) then I got .01565, now im trying to calculate the equilibrium pressure of O2 and that has me stumped.
Kp = pO2^1/2
Plug in you value of Kp and solve for pO2.Wouldn't pO2 = (Kp)^2
Yes I would be thank you!!
To find the equilibrium constant (K) and the partial pressure of O2 (PressureO2) at 298K, you need to use the equation and the value of the standard Gibbs free energy change (ΔG°).
The equation you have is:
M2O(s) ⇌ 2M(s) + 1/2O2(g)
The standard Gibbs free energy change (ΔG°) is given as 10.30. This value will help us calculate the equilibrium constant (K).
The relationship between the standard Gibbs free energy change (ΔG°) and the equilibrium constant (K) can be described by the equation:
ΔG° = -RTlnK
Where:
ΔG° = standard Gibbs free energy change
R = gas constant (8.314 J/(mol·K))
T = temperature in Kelvin
Let's assume that R = 8.314 J/(mol·K) and T = 298K.
Substituting these values into the equation, we have:
10.30 = -8.314 × 298 × lnK
Now, we can solve for lnK:
lnK = 10.30 / (-8.314 × 298)
lnK ≈ -0.0042
To find K, we need to take the exponential of both sides:
K = e^(lnK)
K ≈ e^(-0.0042)
K ≈ 0.9958
So, the equilibrium constant (K) at 298K is approximately 0.9958.
To find the partial pressure of O2 (PressureO2) at 298K, we can use the equation relating the equilibrium constant (K) to the partial pressures of the reactants and products.
For the given equation:
M2O(s) ⇌ 2M(s) + 1/2O2(g)
The equilibrium expression, based on partial pressures, is:
K = (PressureO2)^(1/2) / (PressureM)^2
Where PressureO2 is the partial pressure of O2, and PressureM is the partial pressure of the generic metal.
Since the stoichiometric coefficient of O2 is 1/2 in the balanced equation, the value of PressureO2 can be obtained by taking the square root of K:
PressureO2 = √K
PressureO2 = √0.9958
PressureO2 ≈ 0.9979
Therefore, the partial pressure of O2 (PressureO2) at 298K is approximately 0.9979.