# 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)(a) What mass of LP gas is necessary to heat 1.6 L of water from room temperature 25.0°C to 100.0°C? Assume that during heating, 14% 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
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###### FREE Expert Solution

Recall that heat can be calculated using the following equation:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{∆}}{\mathbf{T}}}$

q = heat, J

+qabsorbs heat
–qloses heat

m = mass (g)
c = specific heat capacity = J/(g·°C)
ΔT = Tf – Ti = (°C)

Calculate the mass of LP gas:

92% (434 ratings)
###### 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)

(a) What mass of LP gas is necessary to heat 1.6 L of water from room temperature 25.0°C to 100.0°C? Assume that during heating, 14% of the heat emitted by the LP gas combustion goes to heat the water. The rest is lost as heat to the surroundings.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Heat Capacity concept. You can view video lessons to learn Heat Capacity Or if you need more Heat Capacity practice, you can also practice Heat Capacity practice problems .

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Based on our data, we think this problem is relevant for Professor Marin's class at UCF.

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