Final answer:
To calculate the heat energy to raise the temperature of 20 liters of water from 5°C to 35°C, multiply the water's mass (20,000 g) by the specific heat capacity of water (4.184 J/g°C) and the temperature change (30°C), which results in 2,510,400 J.
Step-by-step explanation:
Calculating the Required Heat Energy
To determine the quantity of heat energy needed to heat 20 liters (20,000 grams) of water from 5°C to 35°C, we will use the specific heat capacity equation. The specific heat capacity of water is 4.184 J/g°C. The formula to calculate the heat energy (Q) is Q = mcΔT, where 'm' is the mass of water in grams, 'c' is the specific heat capacity, and ΔT is the change in temperature in degrees Celsius. For 20 liters of water (which is 20,000 g, since the density of water is approximately 1 g/mL), and the temperature change (ΔT) of 30°C (from 5°C to 35°C), the energy required would be calculated as follows: Q = 20,000 g * 4.184 J/g°C * (35°C - 5°C) Q = 20,000 g * 4.184 J/g°C * 30°C Q = 2,510,400 J Therefore, approximately 2,510,400 joules of energy are needed to heat the 20 liters of water by 30°C.