Ethanol is manufactured by reacting ethene gas and steam in the presence of phosphoric(V)
C2H4(g) + H2O(g) C2H5OH(g) ∆H = –45kJ mol–1
The reaction is carried out at 570K and 60atm.
What would be the consequences of carrying out the reaction at the same temperature but at a
pressure of 200atm?
1 The manufacturing costs would increase.
2 The maximum yield at equilibrium would be higher.
3 The reaction would proceed at a faster rate.
in this question option 123 are correct but i couldnt understand why option 3 is correct?
- davidLv 76 months agoFavorite Answer
Pressure === higher pressure means the molecules are forced into a smaller space, so there will be more collisions, this causes a faster rate of reaction