If the aluminum block is initially at 25 °C, what is the final temperature of the block after the evaporation of the alcohol, assuming the heat required for the vaporization of the alcohol comes only from the aluminum block?

• A. 30 °C
• B. 20 °C
• C. 25 °C
• D. 15 °C

Answer: (D)

Verified step by step guidance

1. Identify the heat transfer process: The heat required for the vaporization of the alcohol is absorbed from the aluminum block, causing its temperature to decrease.
2. Use the formula for heat transfer: \( q = m \cdot c \cdot \Delta T \), where \( q \) is the heat absorbed or released, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the change in temperature.
3. Determine the heat of vaporization for the alcohol: This value is needed to calculate the total heat absorbed by the alcohol during vaporization.
4. Set up the equation: The heat lost by the aluminum block (\( q_{aluminum} = m_{aluminum} \cdot c_{aluminum} \cdot (T_{final} - T_{initial}) \)) is equal to the heat gained by the alcohol (\( q_{alcohol} = m_{alcohol} \cdot \Delta H_{vaporization} \)).
5. Solve for the final temperature \( T_{final} \) of the aluminum block by rearranging the equation and substituting the known values.