# 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?

###### FREE Expert Solution

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.

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

91% (26 ratings) ###### 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?