Final answer:
The heat energy required to raise the temperature of 5000 g of water from 22°C to 100°C is 1,631,280 J or 1.631 MJ, using the specific heat capacity of water.
Step-by-step explanation:
The student's question is about calculating the amount of heat energy required to raise the temperature of a given mass of water from one temperature to another. To solve this problem, we use the specific heat capacity formula: q = mcΔT, where 'q' is the heat energy, 'm' is the mass, 'c' is the specific heat capacity, and 'ΔT' is the change in temperature.
In this case, the soup pot contains 5000 g (5 kg) of water that needs to be brought from 22 °C to 100 °C, so the temperature change (ΔT) is 100 °C - 22 °C = 78 °C. The specific heat capacity of water (c) is 4.184 J/g°C.
Using the formula, we get q = (5000 g) × (4.184 J/g°C) × (78 °C) = 1,631,280 J or 1.631 MJ (megajoules). This is the amount of heat energy that must be added to the water to achieve the desired temperature increase, assuming no heat loss to the surroundings.