# Problem: The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain:2 SO2(g) + O2(g) ⇌ 2 SO3(g)If the equilibrium partial pressures of SO2, O2 and SO3 are 0.564 atm, 0.102 atm and 0.333 atm, respectively at 1000 K, what is Kp at this temperature?A. 0.292 B. 3.42 C. 5.79 D. 8.11E. 6.05

###### FREE Expert Solution

We’re being asked to determine the equilibrium constant (Kp) at 1000 K for this reaction:

2 SO2(g) + O2(g) ⇌ 2 SO3(g)

Recall that the equilibrium constant is the ratio of the products and reactants

We use Kp when dealing with pressure and Kc when dealing with concentration:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{products}}}{{\mathbf{P}}_{\mathbf{reactants}}}}$     $\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{\left[}\mathbf{products}\mathbf{\right]}}{\mathbf{\left[}\mathbf{reactants}\mathbf{\right]}}}$

Note that solid and liquid compounds are ignored in the equilibrium expression.

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###### Problem Details

The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain:

2 SO2(g) + O2(g) ⇌ 2 SO3(g)

If the equilibrium partial pressures of SO2, O2 and SO3 are 0.564 atm, 0.102 atm and 0.333 atm, respectively at 1000 K, what is Kp at this temperature?

A. 0.292

B. 3.42

C. 5.79

D. 8.11

E. 6.05

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Cook's class at UB.