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### HW 8.53

Posted: Wed Jan 18, 2017 9:25 pm
Why is it that q(reaction) + q(calorimeter)=0 ?

### Re: HW 8.53

Posted: Wed Jan 18, 2017 11:03 pm
Since this is a bomb calorimeter, heat can't go in and out of the system (it's isolated). Therefore heat(q) of the entire system is 0. Therefore any heat lost by an exothermic reaction will warm up the calorimeter, or any heat absorbed by an endothermic reaction will come from the calorimeter and cool it down because there is nowhere else for this heat to go or come from. So the heat change of the reaction is equal and opposite to the heat change of the calorimeter, meaning their sum is 0.

### Re: HW 8.53

Posted: Sat Jan 21, 2017 8:29 pm
So essentially no heat leaves or enters the calorimeter, it is just that the heat is absorbed or given off within the isolated system? Please correct me if I am wrong, I was a little confused by that as well.

### Re: HW 8.53

Posted: Mon Jan 23, 2017 11:54 pm
Another important thing to remember is that q will always equal 0 in an adiabatic process in a closed system. q cannot be negative or positive because no heat is added or removed.