A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20 C. After stirring, the final temperature of both copper and water is 25 C Assuming no heat losses, and that the specific heat (capacity) of water is 4.18 J (gK), what is the heat capacity of the copper in J/K?

I worked this earlier. If you can't find it I will look for a link.

To find the heat capacity of the copper in joules per kelvin (J/K), we can use the principle of energy conservation and the formula for heat transfer:

heat gained by the water = heat lost by the copper

The formula for heat transfer is:

Q = mcΔT

where Q is the heat transferred, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, the copper loses heat, so we'll use a negative sign for its heat transfer:

Q_copper = -Q_water

First, let's calculate the heat transferred by the water:

Q_water = mcΔT
Q_water = (50.0 g)(4.18 J/(gK))(25 - 20) K
Q_water = (50.0 g)(4.18 J/(gK))(5) K
Q_water = 1045 J

Now, using the fact that the copper loses the same amount of heat:

Q_copper = -1045 J

To find the heat capacity of the copper, we divide the heat transfer by the change in temperature:

heat capacity of copper = Q_copper / ΔT
heat capacity of copper = -1045 J / (25 - 100) K
heat capacity of copper = -1045 J / (-75) K
heat capacity of copper = 13.93 J/K

Therefore, the heat capacity of the copper is approximately 13.93 J/K.