To determine which substance experiences the least temperature increase when 500 J of energy is added to 1 kg of each sample, we can use the formula for temperature change:
\[ \Delta T = \frac{Q}{m \cdot c} \]
Where:
- \(\Delta T\) is the temperature increase,
- \(Q\) is the energy added (in joules),
- \(m\) is the mass (in kg), and
- \(c\) is the specific heat capacity (in J kg\(^{-1}\) K\(^{-1}\)).
For each of the given substances with 1 kg mass and \(Q = 500\) J, we can calculate the temperature increase:
-
Aluminum: \[ \Delta T = \frac{500}{1 \cdot 900} = \frac{500}{900} \approx 0.556 , \text{K} \]
-
Copper: \[ \Delta T = \frac{500}{1 \cdot 390} = \frac{500}{390} \approx 1.282 , \text{K} \]
-
Brass: \[ \Delta T = \frac{500}{1 \cdot 380} = \frac{500}{380} \approx 1.316 , \text{K} \]
-
Silver: \[ \Delta T = \frac{500}{1 \cdot 230} = \frac{500}{230} \approx 2.174 , \text{K} \]
-
Platinum: \[ \Delta T = \frac{500}{1 \cdot 130} = \frac{500}{130} \approx 3.846 , \text{K} \]
Now comparing the temperature increases:
- Aluminum: 0.556 K
- Copper: 1.282 K
- Brass: 1.316 K
- Silver: 2.174 K
- Platinum: 3.846 K
The substance that experiences the least temperature increase when 500 J of energy is added is Aluminum.
Thus, the correct response is: A. Aluminum