Industrial chemistry help?!?!?
Hi, I need help with this question:
Another method for the industrial production of ethanol involves the acid catalysed addition of water to ethene as shown here.CH2CH2(g) + H2O(g) ⇆ CH3CH2OH(g) ∆H = -45kJThe industrial synthesis of ethanol by this reaction is conducted at a pressure of around 60-70 atm. How does this choice of pressure affect the rate of attainment of equilibrium? Use your knowledge of collision theory to justify your answer.
- 冷眼旁觀Lv 78 months agoFavourite answer
CH₂CH₂(g) + H₂O(g) ⇌ CH₃CH₂OH(g)
A pressure of around 60-70 atm would give a faster rate of attainment of equilibrium than atmospheric pressure.
Explanation according to collision theory:
At a higher pressure, the gaseous molecules collide more frequently. This lead to faster reaction rates for both of the forward and backward reactions. Therefore, equilibrium would be attained in a shorter time.
- Bobby_ThinLv 78 months ago
The effects of changes in pressure can be described as the increase in pressure will shift the equilibrium towards the side of the reaction with fewer moles of gas.
CH2CH2(g) + H2O(g) ⇆ CH3CH2OH(g)
In your reaction you have more moles on the reactant side so increasing the pressure will move the equilibrium to the right and the formation of product ... hence the high pressure