🤓 Based on our data, we think this question is relevant for Professor Randles' class at UCF.

**When dealing with equilibrium:**

• **K _{c} **→ equilibrium units are in molarity

•

**K _{p} and K_{c} are related to one another by the following equation below: **

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}{{\mathbf{K}}}_{{\mathbf{c}}}{\left(\mathbf{RT}\right)}^{\mathbf{\u2206}\mathbf{n}}}$

**Reaction:**

2SO_{2}(g) + O_{2}(g) ⇌ 2SO_{3}(g)

reactants = 3 moles gas

products = 2 moles gas

Δn = 2 mol – 3 mol**Δ****n = -2**

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}{{\mathbf{K}}}_{{\mathbf{c}}}{\left(\mathbf{RT}\right)}^{\mathbf{\u2206}\mathbf{n}}}\phantom{\rule{0ex}{0ex}}{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\left(\mathbf{1}\mathbf{.}\mathbf{7}\mathbf{\times}{\mathbf{10}}^{\mathbf{8}}\right){\left[\left(\mathbf{0}\mathbf{.}\mathbf{08206}\right)\left(\mathbf{600}\right)\right]}^{\mathbf{-}\mathbf{2}}\phantom{\rule{0ex}{0ex}}{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\left(\mathbf{1}\mathbf{.}\mathbf{7}\mathbf{\times}{\mathbf{10}}^{\mathbf{8}}\right)\left(\mathbf{4}\mathbf{.}\mathbf{13}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{4}}\right)$

**K _{p} = 7.0 x 10^{4}**

An engineer examining the oxidation of SO _{2} in the manufacture of sulfuric acid determines that K_{c} = 1.7 x 108 at 600 K:

2SO_{2}(g) + O_{2}(g) ⇌ 2SO_{3}(g)

(a) At equilibrium, PSO_{3} = 300. atm and PO_{2} = 100. atm. Calculate PSO_{2}.

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Based on our data, we think this problem is relevant for Professor Randles' class at UCF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.