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

Determine the mass of CO_{2} produced by burning enough of methane to produce 2.25x10^{2} kJ of heat.

CH_{4}(g) + 2 O_{2}(g) → CO_{2}(g) + 2 H_{2}O(g); ΔH˚_{rxn}= -802.3 kJ

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