Question

When 5g of C5H10 is burned in a calorimeter (bomb), the temperature of the calorimeter increases by 6 C. If the calorimeter contains 300g of water with a specific heat 4.184kJ/gC, and the calorimeter has an empty heat capacity of 1100J/C, calculate:
A: heat change for SgC5H10
B: Heat of combustion of C5H10

Answer 1

I started with this:
q(system) = - q(reaction)
surroundings = water + calorimeter
q(water) = mass x Change in Temperature ( =6) x 4.184
=7513J
q(calorimeter) = HC (heat capacity=1100) x Change in Temp (=6)
=6600J

q(reaction) = -[ q(water) + q(calorimeter) ] = -14131 J == -14 kJ
Now, I'm going to find the heat combustion for 1 mole of C5H10:
1 mol C5H10 = 70.15g
Heat of combustion = (-14kJ*70.15) / 5g = -19.8kJ for C5H10.

So, for SgC5H10 would I just find heat of reaction for SgC5H10?

Answer 2

you already did! -14kJ