Final answer:
The number of liters of water that must be expended to absorb the energy released by burning 1.00 L of crude oil is approximately 0.00148 L. Crude oil being less dense than water presents additional difficulties in extinguishing a fire on a crude oil tanker.
Step-by-step explanation:
To calculate the number of liters of water that must be expended to absorb the energy released by burning 1.00 L of crude oil, we need to consider the heat transfer to raise the temperature of the water from 20.0°C to 100°C and then to raise the resulting steam's temperature to 300°C.
To raise the temperature of water from 20.0°C to 100°C, we can use the specific heat capacity of water:
Q = mcΔT
Q = (1.00 kg)(4.18 J/g°C)(100°C - 20.0°C)
Q = 3348 J
In order to convert J to liters of water, we need to convert from joules to calories:
1 calorie = 4.184 J
3348 J ÷ 4.184 J/cal = 800.29 cal
Next, we need to calculate the energy required to raise the temperature of water to its boiling point and then to convert the water to steam:
Q = mL
800.29 cal = L(540 cal/g)
L = 1.48 g = 0.00148 kg
Finally, we need to calculate the energy required to raise the temperature of the steam from 100°C to 300°C:
Q = mcΔT
Q = (0.00148 kg)(2.03 J/g°C)(300°C - 100°C)
Q = 222.29 J
Therefore, the number of liters of water that must be expended to absorb the energy released by burning 1.00 L of crude oil is approximately 0.00148 L.
In addition to the difficulty in extinguishing a fire on a crude oil tanker, another complication is that crude oil is less dense than water. This means that it floats on top of the water, exposing it to the oxygen in the air which it uses to burn. Also, if the water is underneath the oil, it is less efficient in absorbing the heat generated by the oil.