Final answer:
To heat a 1-liter pot of water from 20°C to 100°C, one would need 334,720 Joules of energy, which is equivalent to 80 kilocalories.
Step-by-step explanation:
To calculate how much energy is required to bring a 1.0-liter pot of water at 20°C to 100°C, we can use the specific heat capacity of water. The specific heat of water is 4.184 J/g°C. One liter of water has a mass of approximately 1000 grams (1 kg), so we need to consider this mass in our calculation.
First, calculate the temperature change: ΔT = 100°C - 20°C = 80°C.
Then, we use the formula: Energy (Q) = mass (m) × specific heat (c) × temperature change (ΔT).
Therefore, Q = 1000 g × 4.184 J/g°C × 80°C = 334,720 J
To convert joules to kilocalories (kcal), we use the conversion factor that 1 kcal = 4184 J. So, Q = 334,720 J ÷ 4184 J/kcal = 80 kcal.