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Johnson Thai 1L
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Joined: Wed Sep 21, 2016 2:59 pm


Postby Johnson Thai 1L » Tue Mar 14, 2017 8:42 pm

The reaction 2 SO2(g) + O2(g) --> 2 SO3(g) occurs at 25 degrees Celsius and 1 atm in a constant pressure cylinder. Initially, 0.030 mol SO2 and 0.030 mol O2 are present in the cylinder.
Part C asks "Assuming that the reaction goes to completion and that the temperature and pressure of the reaction remain constant, what is the final volume of the cylinder (include any excess reactant)?"
The limiting reactant of the reaction is SO2, so as a result, wouldn't all the SO2 be used up by the end of the reaction, leaving 0.015 mol O2 in excess? The solution manual states that 0.030 mol of SO2 and 0.015 mol of O2 are left in excess. Someone help me explain, thank you!

Posts: 12
Joined: Wed Sep 21, 2016 2:55 pm

Re: #8.101.c

Postby Cherry_Deng_1K » Wed Mar 15, 2017 7:59 pm


I think you misread. The solution manual says 0.030 mol SO3 and 0.015 mol O2 will remain in the container, which makes sense. You are correct that SO2 is the limiting reactant, so all 0.030 mol of SO2 will be used up and converted to 0.030 mol SO3, with 0.015 mol O2 remaining. Therefore, there are 0.045 mol of gas in the container at the end of the reaction.

Ece Ograg 3C
Posts: 5
Joined: Wed Sep 21, 2016 2:55 pm

Re: #8.101.c

Postby Ece Ograg 3C » Fri Mar 17, 2017 12:20 pm

Can someone explain the part E of the same question?
Part E asks: How much enthalpy is exchanged, and does it leave or enter the system?

Return to “Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)”

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