Hi teatea!!
There are a couple of ways in which we can shift the equilibrium of
the production of CH3OH (g).
One is to increase the pressure: during the production of CH3OH the
number of gas molecules decreases (we obtain one mol from 3 moles).
Remember: "If a system is at equilibrium and the pressure is
increased, the
reaction will try to lessen the pressure by shifting to the side with
the lesser number of gas molecules."
There are more moles on the left side of the equation, then by
increasing the pressure during the reaction would increase the rate of
reaction. The number of mole on the left side would react more to
counteract the stress put on the system. This means a shift to the
right because for every CH3OH molecule made, 3 molecules are used up.
The lesser the total number of gas phase molecules in the container,
the lesser the pressure.
This is an exothermic reaction, so another way to improve the yield
would be to carry out the reaction under low temperatures. If we lower
the temperature (heat is removed from the system), the equilibrium
will move to the right in an attempt to raise it again. The system
will try to generate more heat in order to try to replace the heat
lost; the reaction will shift to the right to generate more heat and
in consequence more CH3OH will be produced.
The correct answer is d: decrease the T and increase the P.
Hope this helps you. Feel free to ask for a clarification if it
needed.
Best Regards.
livioflores-ga |
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