Copper has a specific heat of 0.387 J/g·°C. How much energy is required to raise the temperature of 460. g of copper from 34.5°C to 232.0°C?
(460 x 0.387) (232.0 - 34.5)
= 178.02 (197.5)
= 35158.95 J
To calculate the amount of energy required to raise the temperature of a substance, you can use the formula:
q = m * c * ΔT
Where:
q is the amount of heat energy (in Joules)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in J/g·°C)
ΔT is the change in temperature (in °C)
In this case, we have:
m = 460.0 g
c = 0.387 J/g·°C
ΔT = 232.0°C - 34.5°C = 197.5°C
Plugging in these values into the formula, we get:
q = 460.0 g * 0.387 J/g·°C * 197.5°C
Calculating this, we find that the amount of energy required is:
q ≈ 35843.35 J
Therefore, it would require approximately 35,843.35 Joules of energy to raise the temperature of 460.0 g of copper from 34.5°C to 232.0°C.