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When one mole of C6H6 is burned, 3.27 MJ of heat is produced. When the heat from burning 7.21 g of C6H6 is added to 5.69 kg of water at 21.0°C, what is the final temperature of the water?
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7.21 g is 7.21/(6*1+6*12) = 0.092 mol.
It yields 0.092 * 3.27 MJ = 302 kJ
Heating the water with it will give a temperature rise of
302E3 / (5.69*4.2E3) = 12.6 K
21.0°C + 12.6 K = 33.6 °C
one mole of C6H6=78g therefore 7.21g yield 0.3022MJ(7.21/78*3.27) this is energy to raise temp
Q=m c dt m=5.69Kg c=4184 J/KgC Q=0.3022 e^6 .calculate dt
we get dt=12. therefore final temp= 21+12= 33 C