Final answer:
To raise the temperature of 10 g of iron by 1°C requires 4.49 J, whereas for aluminum it requires 9 J. Thus, more energy is needed for aluminum due to its higher specific heat capacity.
Step-by-step explanation:
The amount of energy required to raise the temperature of a substance is determined by its mass, the temperature change, and its specific heat capacity. The formula to calculate this energy, also known as heat, is q = mcΔT, where q is the heat in joules, m is the mass in kilograms, c is the specific heat capacity in J/(kg·°C), and ΔT is the temperature change in Celsius. For iron, which has a specific heat capacity of 0.449 J/g·°C, the energy required to raise the temperature of 10 g by 1°C is (0.449 J/g·°C) × (10 g) × (1°C) = 4.49 J. For aluminum, with a specific heat capacity of 900 J/kg·°C, the energy required is (900 J/kg·°C) × (0.01 kg) × (1°C) = 9 J. Therefore, it takes more energy to raise the temperature of 10 g of aluminum by 1°C than it does for 10 g of iron.