Methanol Purification Version – Daily Question 20200531

Methanol is produced by the reaction of carbon monoxide, carbon dioxide, and hydrogen, as shown in the following equations: CO + 2H2 = CH3OH + Q; CO2 + 3H2 = CH3OH + H2O + Q. According to these equations, the equivalent ratio of hydrogen to carbon monoxide for producing methanol is 2, while the equivalent ratio to carbon dioxide is 3. When both gases are present, the required hydrogen-to-carbon ratio for the feed gas can be expressed as follows: f = H2/CO / (CO + CO2) = 2.1–2.15; m = H2/CO + 1.5CO2 = 2.0–2.05. The composition of the feed gas obtained using different raw materials and processes often deviates from these values. In actual production, the controlled hydrogen-to-carbon ratio should be slightly higher than the stoichiometric ratio. An excess of hydrogen gas plays a beneficial role in extending the catalyst's service life.

Methanol is produced by the reaction of carbon monoxide, carbon dioxide, and hydrogen, as shown in the following equations: CO + 2H2 = CH3OH + Q; CO2 + 3H2 = CH3OH + H2O + Q. According to these equations, the equivalent ratio of hydrogen to carbon monoxide for the synthesis of methanol is 2, while the equivalent ratio to carbon dioxide is 3. When both gases are present, the required hydrogen-to-carbon ratio for the feed gas can be expressed in two ways: f = H2/CO/(CO + CO2) = 2.1–2.15; m = H2/CO + 1.5CO2 = 2.0–2.05. The composition of the feed gas obtained using different raw materials and processes often deviates from these values. In actual production, the controlled hydrogen-to-carbon ratio should be slightly higher than the stoichiometric ratio. Excess hydrogen plays a beneficial role in extending the service life of the catalyst

Methanol is produced by the reaction of carbon monoxide, carbon dioxide, and hydrogen, as shown in the following equations: CO + 2H2 = CH3OH + Q; CO2 + 3H2 = CH3OH + H2O + Q. According to these equations, the equivalent ratio of hydrogen to carbon monoxide for producing methanol is 2, while the equivalent ratio to carbon dioxide is 3. When both gases are present, the required hydrogen-to-carbon ratio for the feed gas can be expressed in two ways: f = H2/CO / (CO + CO2) = 2.1 – 2.15; m = H2/CO + 1.5/CO2 = 2.0 – 2.05. The composition of the feed gas obtained using different raw materials and processes often deviates from these values. In actual production, the controlled hydrogen-to-carbon ratio should be slightly higher than the stoichiometric ratio. An excess of hydrogen gas plays a beneficial role in extending the catalyst's service life.

Methanol is produced by the reaction of carbon monoxide, carbon dioxide, and hydrogen, as shown in the following equations: CO + 2H2 = CH3OH + Q; CO2 + 3H2 = CH3OH + H2O + Q. According to these equations, the equivalent ratio of hydrogen to carbon monoxide for producing methanol is 2, while the equivalent ratio to carbon dioxide is 3. When both gases are present, the required hydrogen-to-carbon ratio for the feed gas can be expressed in two ways: f = H2/CO / (CO + CO2) = 2.1 – 2.15; m = H2/CO + 1.5/CO2 = 2.0 – 2.05. The composition of the feed gas obtained using different raw materials and processes often deviates from these values. In actual production, the controlled hydrogen-to-carbon ratio should be slightly higher than the stoichiometric ratio. An excess of hydrogen gas plays a beneficial role in extending the catalyst's service life.

The molecular ratio of hydrogen to carbon monoxide for synthetic methanol production is 2:1. However, due to factors such as adsorption on the catalyst surface, it is necessary to have a higher hydrogen content in the reaction gas than the theoretical amount in order to increase the reaction rate. The hydrogen content in the feed gas obtained through different processes using various raw materials does not necessarily follow this ratio; feed gases with a high hydrogen content require the addition of carbon dioxide before or after conversion to adjust the hydrogen-to-carbon ratio. In the crude feed gas produced from heavy oil or coal, the hydrogen-to-carbon ratio is too low; therefore, a carbon monoxide conversion unit is required to adjust the ratio of carbon monoxide to hydrogen, followed by the removal of carbon dioxide. According to the material balance of chemical reactions, the composition of the gas entering the methanol synthesis tower meets the requirements for methanol synthesis as well as the theoretical ratio of the feed gases; that is, (H2–CO2)/(CO+CO2) = 2.15. During operation, a slightly higher hydrogen content should generally be maintained. An excess of hydrogen is beneficial in terms of increasing the reaction rate, as well as in reducing the formation of iron carbonyl and higher alcohols; it also helps to extend the lifespan of the catalyst. Therefore, proper control of the carbon-hydrogen ratio has a significant impact on both the utilization rate of raw materials and the purity of the product.

The molecular ratio of hydrogen to carbon monoxide for synthetic methanol production is 2:1. However, due to factors such as adsorption on the catalyst surface, it is necessary to have a higher hydrogen content in the reaction gas than the theoretical amount in order to increase the reaction rate. The hydrogen content in the feed gas obtained through different processes using various raw materials does not necessarily follow this ratio; feed gases with a high hydrogen content require the addition of carbon dioxide before or after conversion to adjust the hydrogen-to-carbon ratio. In the crude feed gas produced from heavy oil or coal, the hydrogen-to-carbon ratio is too low; therefore, a carbon monoxide conversion unit is required to adjust the ratio of carbon monoxide to hydrogen, followed by the removal of carbon dioxide. According to the material balance of chemical reactions, the composition of the gas entering the methanol synthesis tower meets the requirements for methanol synthesis as well as the theoretical ratio of the feed gases; that is, (H2–CO2)/(CO+CO2) = 2.15. During operation, a slightly higher hydrogen content should generally be maintained. An excess of hydrogen is beneficial in terms of increasing the reaction rate, as well as in reducing the formation of iron carbonyl and higher alcohols; it also helps to extend the lifespan of the catalyst. Therefore, proper control of the carbon-hydrogen ratio has a significant impact on both the utilization rate of raw materials and the purity of the product.

Methanol is produced by the reaction of carbon monoxide, carbon dioxide, and hydrogen, with the following reaction equations: CO + 2H2 ≒ CH3OH; CO2 + 3H2 ≒ CH3OH + H2O. As can be seen from these equations, the molar ratio of hydrogen to carbon monoxide required for synthesizing methanol is 2, while the molar ratio when using carbon dioxide is 3. When both carbon monoxide and carbon dioxide are present, there are two ways to express the hydrocarbon ratio (f or M) in the feed gas: f = (H2 – CO2) / (CO + CO2) = 2.05–2.15, or M = H2 / (CO + 1.5 CO2) = 2.0–2.05. The composition of the feed gas obtained using different processes with various raw materials often deviates from these values of f or M. In production, the optimal carbon-to-hydrogen ratio should be slightly higher than the stoichiometric ratio; according to the stoichiometric ratio, the f value or M value is around 2, and in practice the value is kept slightly above 2, meaning that a slightly higher hydrogen content is maintained. Excess hydrogen plays a beneficial role in reducing the formation of iron carbonyl and higher alcohols, as well as in extending the catalyst’s lifespan.

Methanol is produced by the reaction of carbon monoxide, carbon dioxide, and hydrogen, as shown in the following equations: CO + 2H2 = CH3OH + Q; CO2 + 3H2 = CH3OH + H2O + Q. According to these equations, the equivalent ratio of hydrogen to carbon monoxide for producing methanol is 2, while the equivalent ratio to carbon dioxide is 3. When both gases are present, the required hydrogen-to-carbon ratio for the feed gas can be expressed as follows: f = H2/CO / (CO + CO2) = 2.1–2.15; m = H2/CO + 1.5CO2 = 2.0–2.05. The composition of the feed gas obtained using different raw materials and processes often deviates from these values. In actual production, the controlled hydrogen-to-carbon ratio should be slightly higher than the stoichiometric ratio. An excess of hydrogen gas plays a beneficial role in extending the catalyst's service life.

The molecular ratio of hydrogen to carbon monoxide for synthetic methanol production is 2:1. However, due to factors such as adsorption on the catalyst surface, it is necessary to have a higher hydrogen content in the reaction gas than the theoretical amount in order to increase the reaction rate. The hydrogen content in the feed gas obtained through different processes using various raw materials does not necessarily follow this ratio; feed gases with a high hydrogen content require the addition of carbon dioxide before or after conversion to adjust the hydrogen-to-carbon ratio. In the crude feed gas produced from heavy oil or coal, the hydrogen-to-carbon ratio is too low; therefore, a carbon monoxide conversion unit is required to adjust the ratio of carbon monoxide to hydrogen, followed by the removal of carbon dioxide. According to the material balance of chemical reactions, the composition of the gas entering the methanol synthesis tower meets the requirements for methanol synthesis as well as the theoretical ratio of the feed gases; that is, (H2–CO2)/(CO+CO2) = 2.15. During operation, a slightly higher hydrogen content should generally be maintained. An excess of hydrogen is beneficial in terms of increasing the reaction rate, as well as in reducing the formation of iron carbonyl and higher alcohols; it also helps to extend the lifespan of the catalyst. Therefore, proper control of the carbon-hydrogen ratio has a significant impact on both the utilization rate of raw materials and the purity of the product.