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Problem: An atmospheric chemist studying the pollutant SO2 places a mixture of SO2 and O2 in a 2.00-L container at 800. K and 1.90 atm. When the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.65 atm. How many moles of SO3 form?

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We’re being asked to determine how many moles of SO3 form from the reaction of SO2 and O2.

Reaction:      SO2 and O2 react to form SO3

SO2(g) + O2(g) → SO3(g)


Balancing the reaction give us:

2 SO2(g) + O2(g) → 2 SO3(g)


We’re going to calculate the moles of SO3 produced using the following steps.

Step 1. Calculate the moles of gas before the reaction
Step 2. Calculate the moles of gas after the reaction
Step 3. Calculate the change of moles (Δngas) of gas before and after the reaction.
Step 4. Calculate the moles of SO3 formed from the reaction.


We will use the ideal gas equation to determine the moles of gas before and after the reaction.

PV=nRT

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Problem Details

An atmospheric chemist studying the pollutant SO2 places a mixture of SO2 and O2 in a 2.00-L container at 800. K and 1.90 atm. When the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.65 atm. How many moles of SO3 form?

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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 Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Dixon's 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.