q(cal)= -q

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Jennifer Lathrop 1F
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Joined: Sat Dec 02, 2017 3:00 am

q(cal)= -q

Postby Jennifer Lathrop 1F » Sun Jan 27, 2019 12:56 pm

Could someone explain why this is an equation? Like how was this derived and when to apply it?

Jaira_Murphy_2D
Posts: 31
Joined: Fri Apr 06, 2018 3:00 am

Re: q(cal)= -q

Postby Jaira_Murphy_2D » Sun Jan 27, 2019 1:38 pm

I'm not exactly sure how it was derived but I know that it means the Heat lost in a reaction is gained by the calorimeter -q= qcal
(- heat required is = + calorimeter constant)

I think it applies to when you are Calibrating the calorimeter: the heat capacity is measured by supplying a quantity of heat and noting the rise in temperature

Jennifer Lathrop 1F
Posts: 71
Joined: Sat Dec 02, 2017 3:00 am

Re: q(cal)= -q

Postby Jennifer Lathrop 1F » Sun Feb 03, 2019 10:56 pm

thank you!


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