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

Titanium reacts with iodine to form titanium(III) iodide, emitting heat, via the following reaction: 2 Ti(s) + 3 I_{2}(g) → 2 TiI_{3}(s); ΔH˚_{rxn}= -839 kJ. Determine the mass of titanium that reacts if 1.61×10^{3} kJ of heat is emitted by the reaction.

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