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States of Matter question
milani:
Hi, can someone please help me with this question?
An atmospheric chemist, studying the pollutant sulfur trioxide (SO3), places a mixture of sulfur dioxide (SO2) and oxygen (O2) in a rigid 4.10 L container at 941 K and 1.65 atm. When the reaction occurs, gaseous sulfur trioxide is formed according to the balanced equation below and the pressure falls to 1.50 atm.
SO2 + ½O2 → SO3
Assuming that the temperature at the end of the reaction returns to its original value, what is the partial pressure of sulfur trioxide (SO3) after the reaction?
sjb:
Where have you got stuck? Why did the pressure drop?
milani:
i am stuck on how to go about solving the question, my teacher didn't really teach us this.
Borek:
PV=nRT is all you need.
How many moles of all gases initially? How many moles off all gases after the reaction?
How does the change relate to the reaction stoichiometry?
milani:
--- Quote from: Borek on October 07, 2021, 01:57:55 PM ---PV=nRT is all you need.
How many moles of all gases initially? How many moles off all gases after the reaction?
How does the change relate to the reaction stoichiometry?
--- End quote ---
Okay, so I find n before the reaction and then after the reaction... so I have two n values now. How do I go about finding the partial pressure? thanks
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