Hydrogen raises the system pressure
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If the system pressure is 0.01 MPa and it needs to be raised to 25 MPa using hydrogen, with the pressurization process being adiabatic and the system temperature maintained at 200°C, how many m3 of hydrogen are required? The volume of the system is 28 m3. The hydrogen production rate from methanol is 1100 standard liters per hour. I hope the experts here can help answer this
According to the ideal gas law, the relationship between the amount of hydrogen in a system and its volume can be determined: PV = nRT, where P is the pressure of the hydrogen in the system, V is the volume of the hydrogen in the system, n is the amount of hydrogen, R is the gas constant, and T is the temperature of the system. Based on the conditions given in the question, we can establish the equation: 0.01 * 28 = n * (8.314 / 1000) * (200 + 273.15). Solving this equation yields the amount of hydrogen in the system, n, as follows: n = 0.01 * 28 / ((8.314 / 1000) * (200 + 273.15)). Next, we need to calculate the increase in the amount of hydrogen required to raise the pressure from 0.01 MPA to 25 MPA. It is assumed here that the amount of hydrogen remains constant during the adiabatic process: Δn = (25 * 28 – 0.01 * 28) / ((8.314 / 1000) * (200 + 273.15)). Finally, we need to convert the amount of gas into a volume: ΔV = Δn * (8.314 / 1000) * (200 + 273.15) / 25. Thus, the volume of hydrogen required is ΔV in cubic meters. .
For hydrogen at 200°C, it is recommended to use ball valves with zero-friction designs.
Thank you to the seniors for their answers. There is one condition I’m not sure affects this equation or not: hydrogen is pressurized from 0.005 MPA to 26.5 MPA using a hydrogen compressor, and then the system is pressurized to 25 MPA using hydrogen. Does the algorithm change in such a case? I hope the seniors can give me more guidance! Thank you!
Ideal gas law PV=nRT