How much heat (in kJ) must be added to a sample of metal weighing 95.6 g for the temperature to change from 30.0 °C to 98.0 °C? The specific heat of the metal is 0.451 J/g°C.

• A. 4.50 kJ
• B. 2.92 kJ
• C. 3.75 kJ
• D. 1.50 kJ

Answer: (B)

Verified step by step guidance

1. Identify the formula for calculating heat transfer: \( q = m \cdot c \cdot \Delta T \), where \( q \) is the heat added, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the change in temperature.
2. Determine the mass \( m \) of the metal sample, which is given as 95.6 g.
3. Identify the specific heat capacity \( c \) of the metal, which is provided as 0.451 J/g°C.
4. Calculate the change in temperature \( \Delta T \) by subtracting the initial temperature from the final temperature: \( \Delta T = 98.0 \text{ °C} - 30.0 \text{ °C} \).
5. Substitute the values into the formula \( q = m \cdot c \cdot \Delta T \) to find the heat \( q \) in joules, then convert the result from joules to kilojoules by dividing by 1000.