How is methanol produced through gasification of coal? What exactly is the process by which methanol is created?

The brief responses are as follows: 1. Before being used to synthesize methanol, syngas must first undergo a shift reaction (the shift ratio is determined by the gas composition and operating parameters), namely: CO + H2O = H2 + CO2. 2. The syngas after the shift reaction is then decarburized to remove some of the CO2, so as to meet the requirements for gas composition in methanol synthesis: f = (H2 – CO2) / (CO + CO2) = 2.05. 3. The main reactions for methanol synthesis involve the reaction of carbon monoxide, carbon dioxide, and hydrogen in syngas to form methanol under certain pressures and in the presence of a catalyst. The basic reaction equations are: CO + 2H2 = CH3OH + Q (this is the main reaction; the methanol produced via this reaction accounts for about 80% of the total output), and CO2 + 3H2 = CH3OH + H2O + Q (the methanol produced via this reaction accounts for about 20% of the total output). The proportion of methanol produced by these two reactions is not fixed and depends on factors such as the gas composition and the properties of the catalyst. 4. In addition to the above two reactions, there are also the following side reactions during methanol synthesis (the amounts of the products formed are very small, and they are all separated in subsequent distillation steps): 2CO + 4H2 = (CH3)2O + H2O; 2CO + 4H2 = C2H5OH + H2O; 4CO + 8H2 = C4H5OH + 3H2O. 5. The origin of the hydrogen-to-carbon ratio of 2.05: f = (H2 – CO2) / (CO + CO2) = 2.05 is an empirical value derived from the mechanisms of gas-solid phase catalytic reactions in Chemical Reaction Engineering, the properties of methanol catalysts, as well as production data. However, based on the reaction equations, we can conclude that f is approximately equal to 2. CO + 2H2 = CH3OH + Q (1) x 2x x CO2 + 3H2 = CH3OH + H2O + Q (2) y 3y y Note: In equation (1), the amount of CH3OH produced is denoted as x (in moles, or volume, the same applies here); in equation (2), the amount of methanol produced is denoted as y. Then in the system, f = (H2 – CO2) / (CO + CO2) = (2x + 3y – y) / (x + y) = 2(x + y) / (x + y) = 2. The above are the results of the calculations. Of course, due to the complex composition of the feed gas, the calculation of the hydrogen-to-carbon ratio is only an approximate value; it serves as an indicative figure for reference during chemical processing. This post was last edited by zjyang168168 on 2007-11-27 11:01.]

CO + 2H2 = CH3OH + Q (the main reaction; methanol produced accounts for about 80% of the total output) CO2 + 3H2 = CH3OH + H2O + Q (methanol produced accounts for about 0% of the total output). What reactions are responsible for the remaining 20%?

Sorry! 0% was a typo; it should be 20%, which has been corrected.

The purpose of the transformation is to produce H2; adjusting the HC ratio. CO + 2H2 = CH3OH (most people consider this to be the main reaction). CO2 + H2O = CH3OH (it seems a professor mentioned this reaction as well). I disagree with the explanation above, which states that the first reaction accounts for 80% and the second for 20%. In fact, the CO2 content in the refined gas produced in the purification section is controlled at around 3%. Where does the claim of 20% come from? Indeed, the CO2 content increased during the transformation process. But in the purification and decarburization stage, CO2 is already flashed off (it is used to produce urea in fertilizer plants, or it can also be sold as liquid CO2). When thinking back about in which factories engineers work, it seems that the difference mentioned for these indicators is quite large.