Worksheet- Calculations involving Specific Heat

Worksheet- Calculations involving Specific Heat 1. For q= m c Δ T : identify each variables by name & the units associated with it. q = amount of heat...

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Worksheet- Calculations involving Specific Heat 1. For q= m ●c ● Δ T : identify each variables by name & the units associated with it. q = amount of heat (J) m = mass (grams) c = specific heat (J/g°C) ΔT = change in temperature (°C) 2. Heat is not the same as temperature, yet they are related. Explain how they differ from each other. Heat is a combination of kinetic energy (measured by temperature) and potential energy. a. Perform calculations using: (q= m ●c ● Δ T) 1. Gold has a specific heat of 0.129 J/(g×°C). How many joules of heat energy are required to raise the temperature of 15 grams of gold from 22 °C to 85 °C? q=? m = 15 g c = 0.129 J/g°C ΔT = 85°C - 22°C = 63°C

b. Determine if it’s endothermic or exothermic 2. An unknown substance with a mass of 100 grams absorbs 1000 J while undergoing a temperature increase of 15 °C. What is the specific heat of the substance? q = 1000 J m = 100 g c=? ΔT = 15°C

q = mc ΔT q = (15 g)(0.129 J/g°C)(63 °C) q = 121.9 J  120 J

c = 0.666667 J/g°C  0.7 J/g°C

Endothermic or exothermic? Endothermic

Endothermic or exothermic? Endothermic

3. If the temperature of 34.4 g of ethanol increases from 25 °C to 78.8 °C, how much heat has been absorbed by the ethanol? The specific heat of ethanol is 2.44 J/(g×°C) q=? m = 34.4 g c = 2.44 J/g°C ΔT = 78.8°C - 25°C = 53.8°C  54 °C

4. Graphite has a specific heat of 0.709 J/(g×°C). If a 25 gram piece of graphite is cooled from 35 °C to 18 °C, how much energy was lost by the graphite? q=? m = 25 g c = 0.709 J/g°C ΔT = 18°C - 35°C = -17°C

q = (34.4 g)(2.44 J/g°C)(54 °C) q = 4532.544 J  4500 J

q = (25 g)(0.709 J/g°C)(-17 °C) q = --301.325 J  -300 J

Endothermic or exothermic? Endothermic

Endothermic or exothermic? Exothermic

5. Copper has a specific heat of 0.385 J/(g×°C). A piece of copper absorbs 5000 J of energy and undergoes a temperature change from 100 °C to 200 °C. What is the mass of the piece of copper? q = 5000 J m=? c = 0.385 J/g°C ΔT = 200°C - 100°C = 100°C

6. 45 grams of an unknown substance undergoes a temperature increase of 38 °C after absorbing 4172.4 Joules. What is the specific heat of the substance? Look at the table on page 513 of your book, and identify the substance. q = 4172.4 J m = 45 g c=? ΔT = 38°C

m= 129.87 g  100 g

c = 2.44 J/g°C  2.4 J/g°C  Ethanol

Endothermic or exothermic? Endothermic

Endothermic or exothermic? Endothermic

7. A 40 g sample of water absorbs 500 Joules of energy. How much did the water temperature change? The specific heat of water is 4.18 J/(g×°C). q = 500 J m = 40 g c = 4.18 J/g°C ΔT = ?

8. If 335 g of water at 65.5 °C loses 9750 J of heat, what is the final temperature of the water? Liquid water has a specific heat of 4.18 J/(g×°C). q = -9750 J m = 335 g c = 4.18 J/g°C ΔT = Tfinal – 65.5 °C

= 2.99 °C  3°C

2.Endothermic or exothermic? Endothermic

Endothermic or exothermic? Exothermic