3.3 Joule (it follows the equation: Heat loss=mass*specific heat*temp. difference)
1.18x10^4j
You look up the specific heat of copper (per mass unit). Then you multiply specific heat x mass x temperature difference.
86000j
0.385 Joules/Gram Celsius is the specific heat of copper. So, q(Joules) = mass * specific heat * change in temperature q = (200 g Cu)(0.385 J/gC)(30 C - 150 C) = - 9240 Joules -------------------------amount of heat dissipation ( answer can be positive )
You are supposed to divide the energy by the product of (mass x temperature difference).
what is the specific heat for copper
How much heat energy is required to raise the temperature of 0.358 of copper from 23.0 to 60.0 ? The specific heat of copper is 0.0920
1.18x10^4j
Water has.
The specific heat of copper is 0.093 cal/g(C°) or 390 J/kg(C°).
This means that copper will not absorb the heat from the water as much as the aluminum. Aluminum will "steal" more heat from the water- which you do not want. You need the heat to stay with the water until it serves its purpose.
If a person ties a piece of copper wire at the end of the exhaust pipe on a vehicle the copper is going to heat up. When the copper heats up it will turn a rainbow of colors.
aluminium
44.9
q = mass * specific heat * change in temperature 428 joules = (mass)(0.385 J/gC)(25o C) = 44 grams copper ============
You look up the specific heat of copper (per mass unit). Then you multiply specific heat x mass x temperature difference.
These are not temperature numbers but specific heat numbers. They mean that it takes 4.184 Joules and 0.387 Joules respectively to raise water and copper of one gram by one degree celsius. So, as you can see, it takes a lot more heat to raise the temperature of water than it does of copper. Water has a very high specific heat.