Heat and Specific Heat Capacity Notes

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Presentation transcript:

Heat and Specific Heat Capacity Notes CP Chemistry Chapter 15

Energy Energy = ability to do work or produce heat Heat = form of energy that flows from warmer to cooler object James Joule was first person to connect energy and heat Joule (J) = metric unit of heat and energy takes 4.184 joules to move 1 kg mass a distance of 1 meter in 1 second

Types of Energy Potential Energy Kinetic Energy energy of position stored in chemical bonds determined by type and number of chemical bonds Kinetic Energy energy of motion formed when chemical bonds are broken

Law of Conservation of Energy Energy is never created nor destroyed but it can change forms Energy is usually lost in the form of heat Example: car engines convert about 37% of energy into movement feel the top of the hood after driving most energy is lost as heat

Measuring Heat Calorie = amount of heat needed to raise the temperature of 1 gram of pure water by 1oC Food calorie = 1000 calories (or 1 kilocalorie) Memorize the following conversions: 1 Calorie = 1000 calories = 1 kilocalorie 4.184 joules = 1 calorie 1000 joules = 1 kilojoule

How to Solve Heat Problems Use Dimensional Analysis (factor-label method) Set up all ratios with units NOT numbers Plug in numbers Multiply everything on top of fractions Multiply everything on the bottom of fractions Divide two numbers to get final answer

Heat Problems Examples Convert 10 calories to joules Convert 10 joules to calories Convert 3000 calories to Calories Convert 10 Calories to kilojoules

Specific Heat Capacity Specific Heat = heat required to raise 1 gram of a substance by 1 oC Every substance has its own specific heat because it has a different arrangement of atoms Substance Specific Heat (J/goC) Water 4.18 Aluminum 0.897 Gold 0.129 Ethanol 2.44

Specific Heat Equation q = C x m x T q = heat (J) C = specific heat capacity (J/goC) m = mass (g) T = change in temperature (oC) T = Final temperature – Initial temperature

Specific Heat Problem #1 If the temperature of 34.3 g of ethanol increases from 25 oC to 78.8 oC, how much heat has been absorbed by the ethanol? The specific heat for ethanol is 2.44 J/goC.

Specific Heat Problem #2 A 155 g sample of an unknown substance was heated from 25 oC to 40 oC. In the process, the substance absorbed 5696 J of energy. What is the specific heat of the substance?

Specific Heat Problem #3 What is the mass of a substance that has a specific heat of 0.449 J/goC and has its temperature in a calorimeter raised from 20 oC to 90 oC when it releases 12,300 J of energy?

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