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

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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

Chemistry
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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?
you already did! -14kJ

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