An equilibrium mixture at 852 K is found to contain 3.61*10^-3 mol/L of SO2, 6.11*10^-4 mol/L of O2, and 1.01*10^-2 mol/L of SO3. Calculate the equilibrium constant Keq, for the reaction where SO2 and O2 are reactants and SO3 is the product.
Equation would be:
2SO2 + O2 <---> 2SO3
so the equilibrium equation would be:
Keq= [1.01*10^-2]^2/[3.61*10^-3]^2[6.11*10^-4]
but what do I do with the 852 K, will it change the answer at the end after I find the Keq, poor does it change the numbers now?
You work this EXACTLY as you did for the previous problem. The 852 never enters into it EXCEPT that the Keq you calculate will be good ONLY for that temperature.
So basically, the temperature is there just to be there?
In the problem, yes. In real day to day work, you must know the temperature for which the K is given because K is different at some other temperature.
So the answer would be 12811.12?
The temperature, 852 K, is necessary to calculate the equilibrium constant (Keq) because Keq is temperature-dependent. The equilibrium constant expression you wrote is correct:
Keq = [SO3]^2 / ([SO2]^2 [O2])
To calculate Keq, you will substitute the concentrations of SO3, SO2, and O2 at equilibrium into this equation. Given the concentrations:
[SO3] = 1.01 * 10^-2 mol/L
[SO2] = 3.61 * 10^-3 mol/L
[O2] = 6.11 * 10^-4 mol/L
Simply plug these values into the equation:
Keq = (1.01 * 10^-2)^2 / (3.61 * 10^-3)^2 * (6.11 * 10^-4)
Now, calculate the numerical value of Keq using these concentration values.
Note: The temperature, 852 K, is not used directly in this calculation. However, it is critical to remember that Keq is temperature-dependent. Any changes in temperature will affect Keq, but in this specific case, the value of Keq will remain the same since there is no mention of temperature changes.