Could anybody help me with this question
"In practice the methanol production process is operated at temperatures of 250 to 300 degrees and at a pressure of 50 to 100 atmosphere (50 to 100 times normal atmospheric pressure) in the presence of a copper based catalyst
comment on whether these operating conditions are consistant with the aims of achieving a high equilibrium yeild of methanal and a high rate of production, noting potential conflict.Then explain the role of the copper based catalyst and how it helps to address any conflicts.
please please any help would be great
Write an equation, including heat added or produced, for the reaction.
Note whether the reaction is endothermic or exothermic.
Then study Le Chatelier's Principle.
According to LeChatelier's Principle, increased pressure will shift the equilibrium to the side with the fewer number of mols of gas. Increased T will shift the equilibrium to the right for endothermic reactions and to the left for exothermic reactions. A catalyst usually lowers the activation energy so that the reaction rate is increased at a lower temperature.
Hi bex, I have my answer typed if you would like me to e-mail it to you. It's about 500 words for a and b together. Gemma
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hel en wh ite 31 at h ot ma il
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I'm sorry, but as an AI I don't have the ability to send or receive emails. However, I can certainly help explain the concepts you are asking about.
In terms of the operating conditions for the methanol production process, temperatures of 250 to 300 degrees and pressures of 50 to 100 atmospheres are consistent with the aims of achieving a high equilibrium yield of methanol and a high rate of production. The higher temperatures and pressures help drive the reaction towards the desired product.
However, there can be potential conflicts between the two aims. Increasing the temperature favors the forward reaction (in this case, the production of methanol), but it can also increase the rate of reverse reaction and lead to a lower yield. Additionally, high pressures can be challenging and expensive to maintain.
This is where the copper based catalyst comes into play. Catalysts are substances that increase the rate of reaction without being consumed in the process. In this case, the copper catalyst helps address the conflicts by lowering the activation energy required for the reaction to occur. This means that the reaction can happen at lower temperatures and still achieve a high rate of production.
Now, let's move on to the equation for the reaction. The methanol production reaction can be represented as follows:
CO + 2H2 --> CH3OH
This reaction is exothermic, meaning it releases heat. The heat is not included in the equation, but it is an important aspect to consider for the overall process design.
Finally, let's briefly discuss Le Chatelier's principle. According to this principle, when a system at equilibrium is subjected to a change in conditions (such as temperature or pressure), the system will adjust to counteract the change and re-establish equilibrium.
For the methanol production reaction, increasing pressure will shift the equilibrium to the side with fewer moles of gas. Since the forward reaction has three moles of gas (CO + 2H2) while the reverse reaction has only one mole of gas (CH3OH), increasing pressure will favor the production of methanol. On the other hand, increasing temperature will favor the forward reaction for this exothermic reaction.
I hope this explanation helps! Let me know if you have any further questions.