Copper has a specific heat of 0.387 J/g·°C. How much energy is required to raise the temperature of 140. g of copper from 17.5°C to 154.0°C?

q = mass x specific heat x delta T.

To find the amount of energy required to raise the temperature of a substance, we can use the formula:

Q = m * c * ΔT

Where:
Q is the amount of 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 = 140.0 g (mass of copper)
c = 0.387 J/g·°C (specific heat capacity of copper)
ΔT = (final temperature) - (initial temperature) = 154.0°C - 17.5°C = 136.5°C

Now, let's calculate the amount of energy required:

Q = 140.0 g * 0.387 J/g·°C * 136.5°C

Q = 7328.55 J

Therefore, the amount of energy required to raise the temperature of 140.0 g of copper from 17.5°C to 154.0°C is approximately 7328.55 joules.