Step 1

**$\mathbf{q}\mathbf{}\mathbf{=}\mathbf{}\mathbf{mc}\mathbf{\u2206}\mathbf{T}\phantom{\rule{0ex}{0ex}}\mathbf{q}\mathbf{}\mathbf{=}\mathbf{}(1.6L\times \frac{1\mathrm{mL}}{{10}^{-3}L}\times \frac{0.998g}{1\mathrm{mL}})(4.18\frac{J}{g\xb7\xb0C})(100.0\xb0C-25.0\xb0C)$**

**q = 500596.8 J**

LP gas burns according to the following exothermic reaction: C_{3}H_{8}(g) + 5 O_{2}(g) → 3 CO_{2}(g) + 4 H_{2}O(g); ΔH˚_{rxn}= -2044 kJ. What mass of LP gas is necessary to heat 1.6 L of water from room temperature (25.0˚C) to boiling (100.0˚C)? Assume that during heating, 16% of the heat emitted by the LP gas combustion goes to heat the water. The rest is lost as heat to the surroundings.

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