Specific Heat Capacity Temperature vs Heat Temperature is

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Specific Heat Capacity

Specific Heat Capacity

Temperature vs. Heat • Temperature is the measurement of the avg. KE of the

Temperature vs. Heat • Temperature is the measurement of the avg. KE of the particles in matter. • Heat energy that flows from a warmer object to a cooler object.

Learning Check A. When you touch ice, heat is transferred from 1) your hand

Learning Check A. When you touch ice, heat is transferred from 1) your hand to the ice 2) the ice to your hand B. When you drink a hot cup of coffee, heat is transferred from 1) your mouth to the coffee 2) the coffee to your mouth 4

Have you ever noticed that on a hot summer day the pool is cooler

Have you ever noticed that on a hot summer day the pool is cooler than the hot cement? OR maybe that the ocean is cooler than the hot sand?

Specific Heat Capacity Specific Heat: The amount of heat required to raise the temperature

Specific Heat Capacity Specific Heat: The amount of heat required to raise the temperature of 1 gram of a substance 1 degree Celsius. Joule-SI unit for work or energy Calorie-A unit of heat and energy equal to the amount of energy requires to raise the temperature of 1 gram of water by 1° Celsius. 1 calorie = 4. 184 J 1, 000 J = 1 KJ 4, 184 J =1 Calorie

Substance Water Ethanol Aluminum Granite Iron Specific Heat J/(g°C) 4. 184 2. 44 0.

Substance Water Ethanol Aluminum Granite Iron Specific Heat J/(g°C) 4. 184 2. 44 0. 897 0. 803 0. 449

Learning Check A. A substance with a large specific heat 1) heats up quickly

Learning Check A. A substance with a large specific heat 1) heats up quickly 2) heats up slowly B. Sand in the desert is hot in the day, and cool at night. Sand must have a 1) high specific heat 2) low specific heat Lecture. PLUS Timberlake 99 10

Equation: q = c x m x ΔT ΔT = Tfinal – Tinitial q

Equation: q = c x m x ΔT ΔT = Tfinal – Tinitial q = the heat absorbed or released c = the specific heat of the substance m = the mass of the sample in grams ΔT = change in temperature

1. ) Copper metal has a specific heat (Cp) of 0. 385 J/g⁰C. Calculate

1. ) Copper metal has a specific heat (Cp) of 0. 385 J/g⁰C. Calculate the amount of heat (J) required to raise the temperature of 22. 8 g of copper from 20. 0⁰C to 875⁰C. q = c x m x ΔT q =. 385 J/g⁰C x 22. 8 g x 875 ⁰C - 20. 0 ⁰C q = 7505. 19 J gained

2) What is the specific heat of a 25. 0 g substance that absorbs

2) What is the specific heat of a 25. 0 g substance that absorbs 493. 4 J, and raises the temperature from 12. 0⁰C to 34⁰C? q = c x m x ΔT 493. 4 J absorbed = c x 25. 0 g x 34 ⁰C - 12. 0 ⁰C c =. 897 J/g⁰C

3) It takes 1, 250 J of energy to heat a certain sample of

3) It takes 1, 250 J of energy to heat a certain sample of pure silver from 12. 0 0 C to 15. 2 0 C. Calculate the mass of the sample of silver. q = c x m x ΔT 1250 J absorbed =. 240 J/g⁰C x m x 15. 2⁰C -12. 0 ⁰C m = 1627 g

Tomorrow… • Be read for a CHECK UP first thing tomorrow! This is how

Tomorrow… • Be read for a CHECK UP first thing tomorrow! This is how I will know if you are: – Doing your homework! – Understand the content – And what we need to review and reinforce going forward! • Now… – Use your checklist for chapter 10 to complete your flashcards, you can also look at questions that we discussed in class today. – We will come up with more flashcards during opening discussion tomorrow.