Produce Methane Via CO2 + H2O ?

In summary, based on Hess's Law, the reversed reaction of methane combustion is endothermic with an enthalpy of +882 kJ. This means that the reaction would require heat to occur, and simply providing enough heat may not be enough as other reactions may also take place. The Sabatier process, which involves reacting carbon dioxide and water with sunlight and catalyst, is a potential method for producing fuel, but finding and synthesizing the appropriate catalyst is challenging. Some people have reported producing methanol and formic acid instead of methane. It may be possible to carry out the reversed-reaction without sunlight and catalyst, but further research is needed to determine the necessary conditions for this to occur.
  • #1
ossamawww
2
0
it is known that the standard combustion enthalpy of methane is -882 kJ/mol

CH4 + 2 O2 --> CO2 + 2 H2O Hc = -882 kJ

based on hess's law, if a reaction is reversed, so does with the enthalpy

CO2 + 2 H2O --> CH4 + 2 O2 Hc = +882 kJ

which makes the reversed reaction become endothermic. if the system provides enough heat for the reaction (+882 kJ) to be absorbed, would the reaction just simply happen ?? or is there anything else to be considered ?

help me please……
 
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  • #3
You should also take in mind that this is not the only possible reaction. Especially you will also get carbon monoxide, CO, and elementary carbon. That's why you will probably never get methane when heating CO2 and water.
 
  • #4
wait…..the enthalpy of sabatier process is negative, while the reversed-reaction above is positive. so i think it is quite different.

if i increase the temperature, the equilibrium will shift to the right (product region). increasing pressure would not affect the equilibrium since the product and reactant region have the same reaction coefficient. and the need of catalyst (?).

i have read about how fuel could be produced if carbon dioxide and water reacted with sunlight + catalyst (it's called 'artificial photosynthesis'), but it's a bit arduous to find and synthesize the appropriate catalyst.

some people reported that they found methanol and formic acid, instead of methane.

i just wanted to know if it's possible to carry out the reversed-reaction without sunlight and catalyst, based on thermochemistry approach, not photochemistry approach. (by provide sufficient heat or find any catalyst maybe ?)

what should i seek ?

thank youuu
 
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  • #5


There are a few other factors to consider in this reaction. The first is that the reaction needs a catalyst in order to occur at a reasonable rate. The most commonly used catalyst for this reaction is nickel, but there are other options as well. Additionally, the reaction will not occur spontaneously at room temperature and pressure. It requires a significant amount of energy input in order to reach the activation energy and start the reaction. This can be achieved through various methods such as heating or using electricity. Finally, the reaction may also be affected by the equilibrium constant, which depends on the temperature and pressure of the system. Overall, while the theoretical enthalpy change may suggest that the reaction should occur, there are other factors that need to be considered in order for the reaction to take place efficiently.
 

1. How is methane produced from CO2 and H2O?

Methane can be produced through a process called methanation, where carbon dioxide (CO2) and water (H2O) are combined in the presence of a catalyst, such as nickel, to form methane (CH4) and oxygen (O2). This reaction can also occur naturally through the process of methanogenesis carried out by certain microorganisms.

2. What is the purpose of producing methane from CO2 and H2O?

The production of methane from CO2 and H2O has the potential to reduce greenhouse gas emissions and provide a renewable source of energy. Methane is also a versatile fuel that can be used for heating, electricity generation, and transportation.

3. How efficient is the process of producing methane from CO2 and H2O?

The efficiency of methane production from CO2 and H2O depends on various factors, such as the type of catalyst used, temperature, and pressure. Generally, the process has a high energy efficiency, with some studies reporting up to 90% conversion of CO2 and H2O into methane.

4. Is producing methane from CO2 and H2O a sustainable solution for reducing carbon emissions?

Yes, producing methane from CO2 and H2O can be considered a sustainable solution for reducing carbon emissions. This is because the process uses carbon dioxide, a greenhouse gas, as a feedstock and produces methane, a cleaner fuel. Additionally, the process can be powered by renewable energy sources, making it a carbon-neutral process.

5. Are there any challenges or limitations to producing methane from CO2 and H2O?

One of the main challenges of producing methane from CO2 and H2O is the high cost of the process. This is due to the need for a catalyst and the energy required to drive the reaction. Another limitation is the availability of suitable CO2 sources, as well as the need for large-scale infrastructure to capture and process the gas. Additionally, the process currently produces small amounts of methane, making it more suitable for niche applications rather than large-scale energy production.

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