Question

A 25.0 g block of copper (specific heat capacity 0.380 J/g･ °C) at 61.0 °C is placed into 500.0 g of water initially at 20.0 °C. What is the change in temperature (in °C) of the copper block

Answer 1

The change in temperature of the copper block is approximately -10.44 °C.

Step-by-step explanation:

To find the change in temperature of the copper block, we can use the equation:

q = mcΔT

Where q is the heat transferred, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

We are given that the initial temperature of the copper block is 61.0 °C and the final temperature is unknown. We also know that the mass of the copper block is 25.0 g and its specific heat capacity is 0.380 J/g･°C. The heat transferred can be calculated using the equation:

q = mcΔT

Substituting the given values:

q = (25.0 g)(0.380 J/g･°C)(ΔT)

Since the copper block loses heat to reach thermal equilibrium with the water, the heat transferred will be negative. The heat transferred can be calculated using the equation:

q = -mcΔT

Substituting the given values:
-mcΔT = (25.0 g)(0.380 J/g･°C)(ΔT)

Simplifying the equation:

-mcΔT = 9.50 g･J/°C

Now we can solve for ΔT:

ΔT = -9.50 g･J/°C / (25.0 g)(0.380 J/g･°C) ≈ -10.44 °C

Therefore, the change in temperature of the copper block is approximately -10.44 °C.