October 17, 2021, 09:27:42 PM
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### Topic: States of Matter question  (Read 515 times)

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#### milani

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• Mole Snacks: +0/-0 ##### States of Matter question
« on: October 06, 2021, 10:20:09 PM »

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

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« Reply #1 on: October 07, 2021, 02:12:44 AM »
Where have you got stuck? Why did the pressure drop?

#### milani

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« Reply #2 on: October 07, 2021, 08:21:08 AM »
i am stuck on how to go about solving the question, my teacher didn't really teach us this.

#### Borek ##### Re: States of Matter question
« Reply #3 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?
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#### milani

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« Reply #4 on: October 07, 2021, 11:23:27 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?

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

#### Borek ##### Re: States of Matter question
« Reply #5 on: October 08, 2021, 02:53:18 AM »
You don't need partial pressures.

This is a simple stoichiometry: if one mole of SO2 reacts, by how many moles does the number of moles of the mixture change?
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#### milani

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« Reply #6 on: October 13, 2021, 11:33:28 AM »
Sorry, i am still a bit confused. Could you please explain the steps to get to the final answer?
« Last Edit: October 13, 2021, 12:00:03 PM by milani »

#### Borek ##### Re: States of Matter question
« Reply #7 on: October 13, 2021, 11:47:13 AM »
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#### milani

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« Reply #8 on: October 13, 2021, 12:13:20 PM »
if one mole of SO2 reacts, by how many moles does the number of moles of the mixture change?
1?

I have found the initial moles of the reaction and the moles of SO3 in the end as well.

#### Borek ##### Re: States of Matter question
« Reply #9 on: October 13, 2021, 01:29:08 PM »
1?

This is not something to guess, you can calculate from the reaction equation.

Assume you have initially - say - 1 mole of SO2 and 5 moles of O2. There is an excess of oxygen. How many moles of both gases together?

Now reaction proceeds to the end. 1 mole of SO2 reacted, there is none left. How many moles of SO3 were produced? How many moles of O2 left? How many moles of both gases together?

What is the difference?

Does this difference depend on the number of moles of SO2 that reacted? If you are not sure - do identical calculations for an initial mixture of 0.5 moles SO2 and 5 moles of oxygen. For 2 moles SO2 in 5 moles of oxygen. Actually any number of moles of SO2 in excess number of moles of oxygen. Do you see a pattern here?

If so, knowing how many moles of the mixture were present the reaction and after the reaction, can you calculate how many moles of SO2 were present initially in the mixture?
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