An equilibrium mixture of the following reaction was found to have [COF2] = 0.255 M and [CF4] = 0.118 M at 1000°C. What is the concentration of CO2?
2 COF2(g) CO2(g) + CF4(g)
Keq = 2.00 at 1000°C
Thanks:)
You REALLY should use an arrow; otherwise we don't know the difference between reactants and products.
2COF2 ==> CO2 + CF4
Keq = 2.00 = (CO2)(CF4)/(COF2)^2
The problem gives (COF2) = 0.255M
The problem gives (CF4) = 0.118M
Substitute those two into Keq and solve for the only unknown of (CO2).
Thanks:)
To determine the concentration of CO2, we can use the equilibrium constant expression and the given concentrations of COF2 and CF4.
The equilibrium constant expression for the given reaction is:
Keq = [CO2] * [CF4] / [COF2]^2
Substituting the given values into the equation:
2 = [CO2] * (0.118 M) / (0.255 M)^2
Rearranging the equation to solve for [CO2]:
[CO2] = 2 * (0.118 M) * (0.255 M)^2
Calculating the value of [CO2]:
[CO2] ≈ 0.0195 M
Therefore, the concentration of CO2 in the equilibrium mixture is approximately 0.0195 M.
To find the concentration of CO2 in the equilibrium mixture, we can analyze the balanced equation and the given equilibrium concentrations of COF2 and CF4.
The balanced equation for the reaction is:
2 COF2(g) ⇌ CO2(g) + CF4(g)
The equilibrium constant (Keq) for the reaction is given as 2.00 at 1000°C. The Keq expression for this reaction is:
Keq = [CO2] * [CF4] / [COF2]^2
We are given the equilibrium concentrations of COF2 and CF4:
[COF2] = 0.255 M
[CF4] = 0.118 M
To find the concentration of CO2, we need to solve for [CO2].
First, substitute the equilibrium concentrations into the Keq expression:
2.00 = [CO2] * 0.118 / (0.255)^2
Rearrange the equation to solve for [CO2]:
[CO2] = 2.00 * (0.255)^2 / 0.118
Now, calculate the value of [CO2]:
[CO2] = 1.102 M
Therefore, the concentration of CO2 in the equilibrium mixture is 1.102 M.