Energy Efficiency Energy Efficiency the percentage of wasted
![Energy Efficiency Energy Efficiency](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-1.jpg)
![Energy Efficiency the percentage of “wasted” energy to productive (output) energy in your isolated Energy Efficiency the percentage of “wasted” energy to productive (output) energy in your isolated](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-2.jpg)
![Energy Efficiency Equation How much energy is required to change the temperature q=m(ΔT)c q=amount Energy Efficiency Equation How much energy is required to change the temperature q=m(ΔT)c q=amount](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-3.jpg)
![Specific Heat A certain number that tells us how much energy is required to Specific Heat A certain number that tells us how much energy is required to](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-4.jpg)
![Back to our equation… q=m(ΔT)c q=amount of energy (measured in Joules) m=mass (measured in Back to our equation… q=m(ΔT)c q=amount of energy (measured in Joules) m=mass (measured in](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-5.jpg)
![Example 2: Randy has a 500 g of water at 20°C. If he wants Example 2: Randy has a 500 g of water at 20°C. If he wants](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-6.jpg)
![Example 3: Harry has a 50 g lump of unknown material. He experiments with Example 3: Harry has a 50 g lump of unknown material. He experiments with](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-7.jpg)
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![Energy Efficiency Energy Efficiency](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-1.jpg)
Energy Efficiency
![Energy Efficiency the percentage of wasted energy to productive output energy in your isolated Energy Efficiency the percentage of “wasted” energy to productive (output) energy in your isolated](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-2.jpg)
Energy Efficiency the percentage of “wasted” energy to productive (output) energy in your isolated system (Inputs) (Outputs) (“Wasted” Energy)
![Energy Efficiency Equation How much energy is required to change the temperature qmΔTc qamount Energy Efficiency Equation How much energy is required to change the temperature q=m(ΔT)c q=amount](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-3.jpg)
Energy Efficiency Equation How much energy is required to change the temperature q=m(ΔT)c q=amount of energy (measured in Joules) m=mass (measured in grams) ΔT= change in temperature (measured in degrees Celsius) c= specific heat (measured in cal/g°C) Δ means “change in”
![Specific Heat A certain number that tells us how much energy is required to Specific Heat A certain number that tells us how much energy is required to](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-4.jpg)
Specific Heat A certain number that tells us how much energy is required to raise 1 gram of a substance’s temperature 1 degree. These numbers will always be the same for that substance. Example: cwater= 1 cal/g°C OR cwater=4. 184 J/g°C calories is the unit specific for heat energy (note: it is a lowercase c… this is important!) We can still use Joules but c is a different number
![Back to our equation qmΔTc qamount of energy measured in Joules mmass measured in Back to our equation… q=m(ΔT)c q=amount of energy (measured in Joules) m=mass (measured in](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-5.jpg)
Back to our equation… q=m(ΔT)c q=amount of energy (measured in Joules) m=mass (measured in grams) ΔT= change in temperature (measured in degrees Celsius) c= specific heat (measured in cal/g°C) Example: How many calories of heat will need to be added to a 200 g sample of water to raise its temperature 30°C? Step 1: Write down your givens: q= ? m= 200 g ΔT= 30°C c=1 cal/g°C Step 2: Rewrite your equation: q=m(ΔT)c Just like 1 Kilogram equals 1000 grams! Step 3: Substitute your givens for all variables possible: q=(200)(30)(1) Step 4: Solve the algebra problem: q=6000 calories OR q=6 Calories (the large “C” is equal to 1000 “c”’s)
![Example 2 Randy has a 500 g of water at 20C If he wants Example 2: Randy has a 500 g of water at 20°C. If he wants](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-6.jpg)
Example 2: Randy has a 500 g of water at 20°C. If he wants the final temperature of the water to be 75°C, how many Joules of heat will he need to add? Step 1: Write down your givens: q= ? m= 500 g ΔT= 75°C-20°C = 55°C c=4. 184 J/g°C Step 2: Rewrite your equation: q=m(ΔT)c To find the CHANGE in the temperature we subtract final temperature minus the initial temperature. We use 4. 184 here because the problem asked for how many JOULES of heat we needed, not calories Step 3: Substitute your givens for all variables possible: q=(500)(55)(4. 184) Just like 1 Kilogram equals 1000 grams! Step 4: Solve the algebra problem: q= 115, 060 Joules OR 115. 06 Kilojoules
![Example 3 Harry has a 50 g lump of unknown material He experiments with Example 3: Harry has a 50 g lump of unknown material. He experiments with](https://slidetodoc.com/presentation_image_h/b1bb574b61f616b538f65ba63afdd9bc/image-7.jpg)
Example 3: Harry has a 50 g lump of unknown material. He experiments with the material and determines that the temperature of the substance increases by 6°C when 20 cal of heat are added. What is the substance’s specific heat? Step 1: Write down your givens: q= 20 cal m= 50 g ΔT= 6°C c=? Step 2: Rewrite your equation: q=m(ΔT)c Step 3: Substitute your givens for all variables possible: 20=(50)(6)(c) Step 4: Solve the algebra problem: 20 = 300 c 300 0. 067 cal/g°C = c