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ipn [44]
3 years ago
7

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 1.21 pounds of butane (fuel value is 10.85 kcal/g) is used to heat 123.0 kg of water at an initial temperature of 18.0 °C, what is the final temperature?
Physics
2 answers:
Nastasia [14]3 years ago
7 0
Convert 1.29 lbs C4H10 to grams = ? 
<span>Then ? g x 10.85 kcal/g = q kcal or 1000q cal. </span>
<span>1000q = mass H2O x specific heat H2O x (Tf-Tinitial) </span>
<span>Solve for Tf. </span>
<span>I estimate the answer is about 71 C</span>
Alex777 [14]3 years ago
4 0

Answer:

66°C

Explanation:

Energy obtained from burning 1.21 pounds of butane gives a fuel value of 10.85 kcal/g

mass of water = 123.0kg

Initial temperature = 18.0°C

Final temperature = α

Energy released from burning butane is used to heat water to the final temperature

Energy released = Q released

Q released = 1.21 * 453.59 * 10.85

= 5954.96J

Energy needed = Q needed

Q needed = 123 * 1 * (α - 18)

= 123(α - 18)

Q needed = Q released

123(α - 18) = 5954.96

α - 18 = 5954.89/123

α - 18 = 48.41

α = 48.41 + 18

α = 66.41

α = 66° C (approximately)

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For this problem we use two equations the equations of the focal distance in mirrors

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          1 / i = 1 / f₂ - 1 / (L-f₁)

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