$\mathbf{\u2206}\mathbf{H}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{q}}{\mathbf{mol}}\phantom{\rule{0ex}{0ex}}\mathbf{q}\mathbf{}\mathbf{=}\mathbf{}\mathbf{\u2206}\mathbf{H}\mathbf{\times}\mathbf{mol}\phantom{\rule{0ex}{0ex}}\mathbf{q}\mathbf{}\mathbf{=}\mathbf{\u2206}\mathbf{H}\mathbf{}\mathbf{\times}\frac{\mathbf{m}}{\mathbf{MM}}$

Consider the following thermochemical equation for the combustion of acetone (C_{3}H_{6}O), the main ingredient in nail polish remover: C_{3}H_{6}O(l) + 4 O_{2}(g) → 3 CO_{2}(g) + 3 H_{2}O(g), ΔH˚_{rxn} = -1790 kJ. If a bottle of nail polish remover contains 177 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL.

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