Final answer:
To solve this problem, we use the ideal gas law to find the final pressure after 2 hours of flight. The answer is (C) (1400) psi G.
Step-by-step explanation:
To solve this problem, we need to use the ideal gas law, which states that PV = nRT. Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. In this case, we have the initial pressure, volume, and temperature, and we need to find the final pressure after 2 hours of flight.
First, we convert the initial pressure from psi G to absolute pressure by adding the atmospheric pressure. So, the initial absolute pressure is (1800 + 14.7) psi.
Next, we convert the initial temperature from Fahrenheit to Kelvin. The conversion formula is: K = (°F - 32) * 5/9 + 273.15. So, the initial temperature is (70 - 32) * 5/9 + 273.15 K.
Using the ideal gas law, we can find the initial number of moles of oxygen by rearranging the equation to n = PV / RT. Substitute the initial values for P, V, and T to find the initial number of moles.
Now, we can calculate the final pressure after 2 hours of flight. Since the pressure reduces by 400 psi G per hour, the final absolute pressure is the initial absolute pressure minus (2 * 400) psi.
To convert the final absolute pressure back to psi G, subtract the atmospheric pressure from the final absolute pressure.
The answer is (C) (1400) psi G.