Moderators: Chem_Mod, Chem_Admin

Nick Fiorentino 1E
Posts: 102
Joined: Wed Sep 18, 2019 12:16 am


Postby Nick Fiorentino 1E » Fri Jan 31, 2020 6:50 pm

In the solution, it shows q(reaction) equal to -q(calorimeter). Why is this? And how do you know when to use this method?

Kassidy Ford 1I
Posts: 103
Joined: Sat Aug 17, 2019 12:16 am
Been upvoted: 1 time

Re: 4A.13

Postby Kassidy Ford 1I » Fri Jan 31, 2020 8:14 pm

just think about the law of conservation of energy. energy cannot be created or destroyed, only transferred. So the positive q(reactants) must have come from a -q(calorimetry).

Posts: 104
Joined: Thu Jul 25, 2019 12:17 am
Been upvoted: 1 time

Re: 4A.13

Postby VPatankar_2L » Fri Jan 31, 2020 8:17 pm

Since diluted aqueous solutions have similar heat capacities as water, you can assume that the heat capacity of the calorimeter is the same as that of the solution. This would allow the qreaction to equal -qcalorimeter.

Bella Townsend
Posts: 50
Joined: Wed Feb 20, 2019 12:18 am

Re: 4A.13

Postby Bella Townsend » Fri Jan 31, 2020 8:44 pm

Due to the law of conservation of energy, the q of the system is equal to the -q of the surroundings. So when you use a bomb calorimeter, you combust the substance inside. Therefore, the q of the substance is equal to the -q of the bomb calorimeter.

Orrin Zhong 4G
Posts: 51
Joined: Sat Jul 20, 2019 12:16 am

Re: 4A.13

Postby Orrin Zhong 4G » Fri Jan 31, 2020 9:11 pm

The heat released from a reaction [q(reaction)] must go somewhere, so it is absorbed by the calorimeter. Therefore, if the temperature of the reaction decreases, then the heat from the reaction will go to the calorimeter, increasing the temperature of the calorimeter. Thus, q(reaction) = -q(calorimeter).

Return to “Heat Capacities, Calorimeters & Calorimetry Calculations”

Who is online

Users browsing this forum: No registered users and 4 guests