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Ghella [55]
2 years ago
15

An aluminum engine block requires 8669 kJ of energy for the temperature to rise from 75.0 °F to 195 °F. The specific heat of lea

d is 0.897 J/(g°C)( What is the mass of the engine in kg? Please note that the temperatures are in °F, and need to be converted to °C.
Chemistry
1 answer:
quester [9]2 years ago
6 0

Answer:

The answer to your question is 144 kg

Explanation:

Data

Q = 8669 kJ

T1 = 75°F

T2 = 195°F

Cp = 0.897 J/(g°C)

m = ?

Formula

           Q = mCp(T2 - T1)

Process

1.- Convert temperature to °C

T1 = (75 - 32) / 1.8

   = 43/1.8

   = 23.9°C

T2 = (195 - 32) / 1.8

     = 163/1.8

     = 90.6°C

2.- Solve for m

            m = Q / Cp(T2 - T1)

3.- Substitution

            m = 8669000 / 0.897(90.6 - 23.9)

4.- Simplification

            m = 8669000 / 59.83

5.- Result

            m = 144893.66 g or 144.9 kg

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What quantity of energy, in joules, is required to raise the temperature of 425 g of tin from room temperature, 25.0 °C, to its
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Answer:

Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is 45.249 kiloJoules.

Explanation:

Mass of the tin ,m= 425 g

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Initial temperature of the tin ,T_1= 25.0 °C = 298.15 K

Final temperature of the tin, T_2= 231.9 °C = 505.05 K

Let the heat required to change the temperature of tin from 298.15 K to 505.05 K be Q.

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Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is:

= Q+Q' =  19.961 kJ + 25.288 kJ = 45.249 kJ

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