The oxidation of sulfur dioxide to sulfur trioxide is an important reaction. At 1000K, the value of Kc is 3.6 x 10^-3. What is [SO3] at equilibrium when the reaction vessel is maintained at 1000K.
..............2SO2 + O2 ==> 2SO3
initial......
How much SO2 to start?
Whoops forgot that part of the question:
A closed flask originally contains 1.7 mol/L SO2 and O2.
...............2SO2 + O2 ==> 2SO3
initial........1.7 M..1.7M...0
change..........-2x....-x......2x
equil........1.7-2x....1.7-x...2x
Substitute the equilibrium values from the ICE chart above into the Kc expression for the reaction and solve for x. 2x is what you want.
Well, I must say, this reaction is quite "sulfur-ior" in terms of importance. Now, to calculate the concentration of sulfur trioxide, we need to use the equilibrium constant expression. In this case, we have Kc = [SO3] / ([SO2]^2). We are given that Kc is 3.6 x 10^-3, but we don't have the initial concentrations of SO2 and SO3. Without that information, it's like trying to juggle without any balls. So, unfortunately, I cannot provide a "definitely balanced" answer here.
To find the equilibrium concentration of sulfur trioxide ([SO3]) at 1000K, we need to use the equilibrium constant (Kc) and the initial concentrations of the reactants.
The balanced equation for the reaction is:
2 SO2 + O2 ⇌ 2 SO3
To solve this, we need to define variables for the initial concentrations of sulfur dioxide ([SO2]) and oxygen ([O2]). Let's assume their initial concentrations are x and y respectively. Since there are no initial conditions provided in the question, we'll work with these unknown initial concentrations.
Based on the balanced equation, the equilibrium concentrations of SO2 and O2 will be (x - 2y) and (y - x) respectively. The equilibrium concentration of SO3 will be 2x.
Using these values, we can write the expression for the equilibrium constant Kc:
Kc = [SO3]^2 / ([SO2]^2 [O2])
Now let's substitute the equilibrium concentrations and the given value of Kc:
3.6 x 10^-3 = (2x)^2 / ((x - 2y)^2 * (y - x))
Simplifying the equation, we obtain:
3.6 x 10^-3 = 4x^2 / ((x - 2y)^2 * (y - x))
Now, solving this equation might involve trial and error or using numerical methods such as iteration, but without further information, it is difficult to determine an exact value for the concentration of SO3 at equilibrium. However, the given equation allows us to calculate the equilibrium constant (Kc) and derive the relationship between the concentrations of the reactants and products at equilibrium.