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6.06 Thermal Energy Calculations

[Place your name here]

On all of these problems, show your work (the numbers that you are using and how you

are using them) and the answer with the proper significant digits and the proper units

where appropriate.

Here is a video that will be helpful with the formulas below.

https://www.khanacademy.org/science/chemistry/states-of-matter-and-intermolecular-

forces/states-of-matter/v/specific-heat-and-latent-leat-of-fusion-and-vaporization-2

Q = m * C * ∆T

Q = m * H

Table 1: Specific Heat of Common Substances

Material

Specific Heat, C (J/kg * K)

Aluminum

900

Copper

390

Ice

2060

Steam

2010

Water

4180

Physics Principles and Problems. Columbus OH: Glencoe/McGraw-Hill., 2009. 318+. Print.

Table 2: Heats of Fusion and Vaporization of Common Substances

Material

Heat of Fusion, H

(J/kg)

Heat of Vaporization, H

(J/kg)

Copper

2.05 x 10

5.07 x 10

Iron

2.66 x 10

6.29 x 10

Water (ice)

3.34 x 10

2.26 x 10

Physics Principles and Problems. Columbus OH: Glencoe/McGraw-Hill., 2009. 318+. Print.

1. How much heat is needed to raise the temperature of 50.0 g of water from 277 K to 315 K?

(5 points)

Mass= 50.0g

ΔT= 315k-277k

ΔT= 38k

specific heat capacity of water, C = 4180 J/kg * K

Q=mcΔT

= 0.05 x 4180 x 38

= 7942J

2. If it takes 1,650 J of energy to raise the temperature of copper from 250 K to 285 K, what is

the mass of the copper? (5 points)

C of Copper= 390 J/kg * K

ΔT=285k-250k

=35k

Heat Energy=1,650 J

M=Q /C ΔT

1,650 J/(35 x 390)= o.12kg

3. A 500 g block of metal absorbs 8,370 J of heat when its temperature changes from 295 K to

338 K. Calculate the specific heat of the metal. (5 points)

M=500g

Heat Energy=8370J

ΔT=338k-295k

=43k

C=Q/m ΔT

C=8370 / (43 x 0.5)

= 389.3023 J/kg * K

4. Use the Specific Heat of Common Substances table to identify the metal in problem 3. (5

points)

389.3023 J/kg * K is the specific heat capacity for Copper

5. How much heat energy is needed to melt 0.300 kg of copper? (5 points)

** Hint: Use the Heat of Fusion

Heat of Fusion= 3.34 x 10

J/kg

q = m·ΔHf

= 0.300 kg x 3.34 x 10

J/kg

q = 100200J

6. How much iron can be vaporized if 1.30 x 10

J of energy is applied? (5 points)

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6.06 Thermal Energy Calculations [Place your name here] On all of these problems, show your work (the numbers that you are using and how you are using them) and the answer with the proper significant digits and the proper units where appropriate. Here is a video that will be helpful with the formulas below. https://www.khanacademy.org/science/chemistry/states-of-matter-and-intermolecularforces/states-of-matter/v/specific-heat-and-latent-leat-of-fusion-and-vaporization-2 Q = m * C * ∆T Q=m*H Q=m*H f v Table 1: Specific Heat of Common Substances Material Specific Heat, C (J/kg * K) Aluminum 900 Copper 390 Ice 2060 Steam 2010 Water 4180 Physics Principles and Problems. Columbus OH: Glencoe/McGraw-Hill., 2009. 318+. Print. Table 2: Heats of Fusion and Vaporization of Common Substances Material Heat of Fusion, H (J/kg) Heat of Vaporization, H (J/kg) f v Copper 2.05 x 1 ...
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