Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: m190908m on March 09, 2018, 06:45:58 PM
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Internal Energy Problem.. A chemical reaction occurs, 25.5 KJ of energy is exchanged between the system and surroundings...
given:
Pressure: 3.50 atm
L*atm= 101.32 J
w= -pDeltaV
temperature change: 7.6 Kelvin
What is the change in internal energy?
This one's really stumping me. Any help would be appreciated. Even just a hint.
I've tried rearranging the pv work equation, I've tried rearranging the change internal equation. Actually just not sure where the temperature fits into all this. I understand most of this. This isn't like any internal energy problem I've run into..
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Here's work
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Side note: I'm not even sure if this problem is possible to solve without more info
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Side note: I'm not even sure if this problem is possible to solve without more info
Thermodynamics is definitely not my forte, but at first sight I don't see how to solve this one as well.
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Doesn't provide enough information to make sense of what's going on. If work is being done, what is moving? Is the reaction being conducted within a piston where ideal gas can be assumed? If so, w = pΔV = nRΔT. What is the direction of the energy exchange in regards to the system and the surroundings?