Problem: LP gas burns according to the following exothermic reaction: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(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.

FREE Expert Solution

Step 1

q = mcTq = (1.6 L×1 mL10-3 L×0.998 g1 mL)(4.18 Jg·°C)(100.0°C-25.0°C)

q = 500596.8 J


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Problem Details
LP gas burns according to the following exothermic reaction: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(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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