Thread Content
The manager asked us technicians to solve a process calculation problem, but everyone came up with different results. Now I’ve posted it online; I’m hoping that experts with extensive experience in this area can take a look at it. Request to list the calculation steps or explain the reason for the answer. Please see below: A calculation regarding the losses associated with carbon dioxide removal from exhaust gases and the hydrogen consumed in the ammonia synthesis process. Conditions: The gas flowing from the third stage of the high-pressure compressor has a volume of 50,000 M3/h. After passing through the carbon dioxide absorption tower, the purity of the gas is such that its CO2 content is 1.6%, and the pressure is 2.0 MPa. This gas is then compressed to 13.0 MPa by the fifth stage of the high-pressure compressor before being sent to the methanol synthesis tower. The reaction equation is: CO2 + 3H2 → CH3OH (methanol) + H2O; in other words, one molecule of H2 is consumed for each molecule of CO2. The conversion efficiency in the synthesis tower is 60%, and 80% of the reactant gas participates in the reaction. If, under all unchanged conditions, the CO2 content in the gas is reduced to 1.5% (a decrease of 0.1%), how many cubic meters of H2 can be saved per day (24 hours)? And what would be the equivalent value in terms of ammonia (NH3) produced? The cost is calculated at 2,200 yuan per ton of ammonia. N2 + 3H2 —— 2NH3 (the equation for ammonia synthesis). This post was last edited by lovefei520 on 2009-4-16 at 19:59