The amount of energy released by burning a fuel source, measured in energy per mass, is called the fuel value. If all the energy obtained from burning 1.26 pounds of methane (fuel value is 11.97 kcal/g) is used to heat 123.5 kg of water at an initial temperature of 18.6 °C, what is the final temperature?
1.00 lbs = 453.592 g
1.26 lbs = 571.5264 g
Given that;
The fuel value of methane is 11.97 kcal/g
So 571.5264 x 11.97 kcal/g = 6841.17 kcal
No this kcal converted into KJ as follows:
1.0 Kcal = 4.184 KJ
6841.17 kcal = 28623.45528 kJ
This amount of energy is used to heat the 123.5 kg water as
follows:
Q = mass *Cp* temperature change
28623.45528 kJ = 123.5 kg x 4.19 kJ/kgoC x Delta T
Delta t = 55.3 oC
If the initial temperature = 18.6 °C,
then the final temperature = 18.6 °C + 55.3 oC
= 73.9 oC
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