For the following combustion reaction CH₂CH₂CH₂COOH(1) + 50₂(g) → 4CO₂(g) + 4H₂O(g) AH = -2.18 x 10³ kJ When a 6.62-g sample of butyric acid (molar mass= 88.10 g/mol) is burned, how much energy (in kJ) is released as heat? 1 4 2 5 KJ 3 6 X C

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