The following reaction is a step in the commercial production of sulfuric acid.

2SO2(g) + O2(g) 2SO3(g)

The equilibrium constant is very high at room temperature, but the reaction is very slow. It must be run at high temperatures to achieve a reasonable rate of reaction. However the equilibrium constant decreases as temperature increases. Calculate Kc at 807 °C from the following concentration data:
[SO3] = 0.016 M
[SO2] = 0.029 M
[O2] = 0.0058 M

I calculated 52.48 for Kc I don't understand how to figure it out for a certain temperature.

You did it at 807C.

so is that the right answer? Because my online assignment keeps telling me that it is incorrect

I didn't work it out

2S02+O2>>2SO3
k=[SO3]^2/[SO2]^2[O2]

I didn't get your answer.

To calculate the equilibrium constant (Kc) at a specific temperature, we need to use the equation:

Kc = ([SO3]^2)/([SO2]^2 * [O2])

First, we substitute the given concentrations into the equation:

Kc = (0.016^2) / (0.029^2 * 0.0058)

Next, we can simplify the equation by performing the calculations:

Kc = 0.000256 / (0.000841 * 0.0058)

Kc = 0.000256 / 0.0000048806

Kc ≈ 52.480

Therefore, the equilibrium constant (Kc) at 807 °C for the given reaction is approximately 52.480.

It is important to note that this calculation assumes ideal gas behavior and that the units of concentration are consistent, such as molarity (M) for all species involved.