10 replies to this topic

[DecadentParadise]

Is it right that the pressure should be high as the product has overall less moles than reactants? Also, i have no idea how to work out whether the reaction is exo/endothermic and therefore what temperature it should be at.. could someone please explain this to me?

[dondon]

Exothermic is when the reaction gives out energy and endothermic is when it takes in energy for use in a reaction but i dont know what the question is i'm assuming its something about equlibrium??

[DecadentParadise]

The question IS about equilibrium.. and i know the definition you've given but its something specific about the question. I was meaning, How do you work out whether its exo/endo from the information given. so you'll have to see the question to help me.

[dondon]

could u not just copy it out if its an equlibrium equation co i dont have past papers

[dfx]

"Also, i have no idea how to work out whether the reaction is exo/endothermic "

Strange, normally they specify its for the forward or reverse reaction, but they haven't.

It IS high pressure because there's 2 moles of gasses on the right hand side (reactants) and 1 mole on the left (products). Increasing the pressure shifts the equilibrium to the side with less moles of gases - which is the products, and so high pressure.

I think you have to know the process is exothermic off by heart from the chemical industry or something... cause they've quoted the DeltaH as +/- 46.

[DecadentParadise]

Lol, i'll give it my best.


Under the conditions used industrially, ethene and steam react as follows.


C2H2(g) + H2O(g) ->/<- C2H5OH(g) /_\H= +/- 46kJmol^+/-1

(Ethene + Steam -> Ethanol)

Which set of conditions would give the best yield of ethanol at equilibrium?

A - High temperature, low pressure
B - High temperature, high pressure
C - Low temperature, high pressure
D - Low temerature, low pressure

As i said, i can work out the pressure part. But am clueless as how to assert the endothermic/exothermic directions in the reaction.

[dondon]

Lol, i'll give it my best.


Under the conditions used industrially, ethene and steam react as follows.

                           
C2H2(g) + H2O(g)    ->/<-    C2H5OH(g)  /_\H= +/- 46kJmol^+/-1
                           
    (Ethene + Steam -> Ethanol)   

Which set of conditions would give the best yield of ethanol at equilibrium?

A - High temperature, low pressure
B - High temperature, high pressure
C - Low temperature, high pressure
D - Low temerature, low pressure

As i said, i can work out the pressure part. But am clueless as how to assert the endothermic/exothermic directions in the reaction.

Bonds are forming in the forward reaction and bonds forming take in energy whereas bonds breaking release energy so the forward reaction is endothermic so its high temperature.

[e-unit]

Lol, i'll give it my best.


Under the conditions used industrially, ethene and steam react as follows.

                            
C2H2(g) + H2O(g)    ->/<-    C2H5OH(g)   /_\H= +/- 46kJmol^+/-1
                           
     (Ethene + Steam -> Ethanol)   

Which set of conditions would give the best yield of ethanol at equilibrium?

A - High temperature, low pressure
B - High temperature, high pressure
C - Low temperature, high pressure
D - Low temerature, low pressure

As i said, i can work out the pressure part. But am clueless as how to assert the endothermic/exothermic directions in the reaction.

Bonds are forming in the forward reaction and bonds forming take in energy whereas bonds breaking release energy so the forward reaction is endothermic so its high temperature.

Its a typo. They would never say mol l^+/- . It doesnt make sense

[Ally]

That questions has a typo. It meant to be -ve.

[dfx]

wow how convenient for leckie and leckie to completely ignore their stupid typos

[Ally]

There is also a typo in question 12 (c ) in the 2000 paper.

The equation is meant to read as:

CH₃NHNH₂(l) + 2.5 O₂ ----> CO₂(g) + 3H₂O(l) + N₂(g)

H = -1305KJmol^-1