: ΔQ = mcΔT : ΔQ = (60g) (0.385 J g−1 K−1) (60 °C same as 60 Kelvin) : :: = 1386 Joules
q = (250 g)(0.46 J/gC)(300 C - 27 C) = 3.1 X 104 Joules -------------------------
The nagle of light determines the area over which the energy of the light is spread out and that will affect how much it is heated.
None. They are 75% copper and 25% copper.
1963 COPPER penny is worth half a billion dollars.
That completely depends on the specific heat capacity of the substance of which the sample is composed, which you haven't identified. It will take a lot more heat energy to raise the temperature of 65 grams of water 35 degrees than it would take to do the same to 65 grams of iron or yogurt, e.g.
Too much heat would result in brake damage, which is absorbed in the brake drum.
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
51%
Solid copper appears to gain mass when heated in air, because the copper reacts with oxygen in the air to form copper oxide. However, the actual mass of the copper does not increase; the mass of the solid increases by a value equal to the mass of oxygen removed from the air.
How much it is heated. What has the heat done to the object ETC
A copper wire is a much better conductor of heat than air is.
q = mHvq = heatm = mass (30g)Hv = heat of vaporization (2,260J/g)q = (30g)(2,260J/g)q = 67,800JWhen 30 grams of water is converted into steam, how much heat is absorbed?67,800J of heat, also represented as 67.8kJ of heat is absorbed.
The specific heat of lead is 0.0305 K cal/kg deg C. The heat absorbed will be 38x(180-26)x0.0305 = 178.5 Kcal = 746.1 K joules
q = (250 g)(0.46 J/gC)(300 C - 27 C) = 3.1 X 104 Joules -------------------------
It depend upon the temperature how much you heat it
all of them, just depends on how much heat you use
It depends how much heat is applied and the mass of the gold.