Final answer:
The energy needed to raise the temperature of 0.40 kg of water from 15°C to 60°C using the specific heat capacity of 4200 J/kg°C is 75,600 J or 75.6 kJ.
Step-by-step explanation:
Calculating Energy Required to Heat Water
To calculate the energy required to raise the temperature of water, the specific heat capacity of water must be used in conjunction with the mass of the water and the temperature change. For the provided question, we need to find the energy to raise the temperature of 0.40 kg of water from 15°C to 60°C. Considering water's specific heat capacity of 4200 J/kg°C, the formula Q = mcΔT where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the temperature change, is applicable.
Plugging in the values, we have: Q = (0.40 kg) × (4200 J/kg°C) × (60°C - 15°C). The temperature change (ΔT) is 45°C. Multiplying these figures, we find that Q equals 75,600 J or 75.6 kJ (1 kJ = 1000 J), which is the energy required to heat the water by the specified temperature range.