r the following combustion reaction CH₃CWhen a 7.52-g sample of butyric acid (molar mass = 88.10 g/mol) is burned, how much energy (in kJ) is released as heat?

Question

For the following combustion reaction CH₃CH₂CH₂COOH(l) + 5O₂(g) → 4CO₂(g) + 4H₂O(g) ∆H = -2.18 × 10³ kJ When a 7.52-g sample of butyric acid (molar mass = 88.10 g/mol) is burned, how much energy (in kJ) is released as heat?

Answer 1

Grams to energy conversion: (formula is (m/M_BA) x ΔH_comb)

7.52 g BA (1 mole/88.10 g BA)(-2.18x10³ kJ/mole BA) = kJ

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