Final answer:
To absorb the energy released by burning 1.00 L of crude oil, approximately 9.35 L of water must be expended. Crude oil is less dense than water, which allows it to float on top and be exposed to oxygen, increasing the risk of combustion.
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 determine the energy transferred to the water. First, calculate the energy required to raise the temperature of the water from 20.0 °C to 100 °C:
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.
Next, calculate the energy required for the water to boil:
Q = mL
Where L is the heat of vaporization.
Finally, calculate the energy required for the steam to rise to 300 °C:
Q = mcΔT
Now, add up all the energy values calculated above to find the total energy that needs to be absorbed. Then, divide this total energy by the energy released by burning 1.00 L of crude oil (2.80 × 10^7 J) to find the number of liters of water required.
The answer is 9.35 L. Therefore, the correct option is (a).
An additional complication caused by the fact that crude oil is less dense than water is that it floats on top of the water. This exposes the oil to oxygen in the air, which can lead to combustion. Additionally, if the water is under the oil, it is less efficient in absorbing the heat generated by the oil.