Problem: An engineer examining the oxidation of SO 2 in the manufacture of sulfuric acid determines that Kc = 1.7 x 108 at 600 K: 2SO2(g) + O2(g) ⇌ 2SO3(g) (a) At equilibrium, PSO3 = 300. atm and PO2 = 100. atm. Calculate PSO2. 

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

FREE Expert Solution

When dealing with equilibrium:

Kc → equilibrium units are in molarity 
Kp → equilibrium units in terms of pressure


Kp and Kc are related to one another by the following equation below: 

Kp=KcRTn


Reaction:

2SO2(g) + O2(g) ⇌ 2SO3(g)

reactants = 3 moles gas

products = 2 moles gas


Δn = 2 mol – 3 mol
Δn = -2


Kp=KcRTnKp=1.7×1080.08206600-2Kp=1.7×1084.13×10-4

Kp = 7.0 x 104


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Problem Details

An engineer examining the oxidation of SO 2 in the manufacture of sulfuric acid determines that Kc = 1.7 x 108 at 600 K: 

2SO2(g) + O2(g) ⇌ 2SO3(g) 

(a) At equilibrium, PSO3 = 300. atm and PO2 = 100. atm. Calculate PSO2

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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 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.