Final answer:
To calculate the energy required to heat 2.5L of water from 20°C to 50°C, use the specific heat capacity formula. The calculation results in 2.5 kg of water needing 313,950 J or 313.95 kJ of energy.
Step-by-step explanation:
To calculate the energy required to raise the temperature of water, you can use the specific heat capacity formula. The formula is Q = mcΔT, where Q is the energy in joules, m is the mass of the water in kilograms, c is the specific heat capacity of water (4.186 J/g°C), and ΔT is the change in temperature in Celsius. First, convert 2.5 liters of water to kilograms. Since the density of water is close to 1 kg/L, 2.5 liters of water is approximately 2.5 kg. Next, calculate the change in temperature (ΔT): 50°C - 20°C = 30°C.
Now, plug the values into the formula to find the energy needed:
Q = (2.5 kg)(4.186 J/g°C)(30°C) = 31,395 J. Since there are 1,000 g in 1 kg, the specific heat capacity will be 4,186 J/kg°C for water. So Q = (2.5 kg)(4,186 J/kg°C)(30°C) = 313,950 J or 313.95 kJ. This is the amount of energy required to heat 2.5L of water from 20°C to 50°C, ignoring heat losses to the environment.