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equilibrium ... again


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#1 xClairex

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Posted 17 January 2007 - 07:35 PM

The industrial preparation of methanol involves the combination of carbon monoxide and hydrogen using a zinc oxide catalyst according to the equation:

CO(g) + 2H2 (two way arrow) CH3OH(g)

a)in industry the reaction is usually carried out at 300 atmospheres pressure. Explain the use of high pressure

b)Is the reaction which produces methanol exothermic or endothermic? Explain



#2 Michael

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Posted 17 January 2007 - 09:00 PM

Hi again,

a) With high pressure the equilibrium will move towards the side with less gas volumes. On the right you have 3 volumes(1 CO and 2H2) whereas on the left there is only one. So it will move towards methanol. Its more economic to do this in industry.

b) I think you're missing some info, does it tell you what the enthalpy value is for either the forward or the reverse reation?

#3 xClairex

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Posted 17 January 2007 - 10:01 PM

nope it doesn't say you are supposed to work it out some how :s


#4 Michael

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Posted 17 January 2007 - 10:36 PM

After having a chat with someone its simpler than I though. In a reaction where bonds are made the compound so you are releasing energy whereas to break bonds you have to put energy into the system. Therefore its exothermic

#5 dfx

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Posted 17 January 2007 - 11:21 PM

QUOTE(xClairex @ Jan 17 2007, 10:01 PM) View Post
nope it doesn't say you are supposed to work it out some how :s


Hess's cycle, if you're supposed to work it out.





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