a 57 g of copper is at 12 degrees celsius, if 1012 J of energy is added to the copper, what is the final temperature of the copper?

Add 1012/(C*M) to 12 degC

C = specific heat of copper, 0.386 J/g*degC

M = 57 g

I get 12 + 46 = 58 deg C

To find the final temperature of the copper, we can use the formula for heat transfer:

Q = m * C * ΔT

Where:
Q = Amount of heat absorbed (in Joules)
m = Mass of the material (in grams)
C = Specific heat capacity of the material (in J/g°C)
ΔT = Change in temperature (final temperature - initial temperature, in °C)

In this case, we know:
Q = 1012 J
m = 57 g
C = Specific heat capacity of copper, which is approximately 0.385 J/g°C (this value can be found in reference books or online)

Let's rearrange the formula to solve for ΔT:

ΔT = Q / (m * C)

Substituting the given values:

ΔT = 1012 J / (57 g * 0.385 J/g°C)

Now let's calculate the change in temperature:

ΔT = 1012 J / (21.945 g°C)

ΔT ≈ 46.09°C

Since the initial temperature is 12°C, we can find the final temperature by adding the change in temperature to the initial temperature:

Final temperature = Initial temperature + ΔT

Final temperature = 12°C + 46.09°C

Final temperature ≈ 58.09°C

Therefore, the final temperature of the copper is approximately 58.09°C.