equilibrium will shift to the side of the equation with the least moles in attempt to reduce pressure
in the haber process
N2+3H2 <--> 2NH3
an increase in pressure causes equilibrium to shift the right because it has the least moles (2 instead of 4)
<--> represents a reversible reaction sign
the forward reaction is favored until a new equilibrium is reached
The reaction wants to shift to the side with fewer moles, so as to balance out with the increased pressure.
The reaction will move in the backwards direction.
It may well change the equilibrium point - depending on the reaction.
Well, it will shift the equilibrium position, depending on the reaction. Increasing pressure shifts the equilibrium to the size with less moles of substance
the reaction makes more reactants
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A decrease in radiative equilibrium temperature
Other aspects of the system (such as heat) will change to maintain equilibrium
decreases
Yes. If the pressure is increased, even with a noble gas, the reaction equilibrium will shift to alleviate and lower that increased pressure (if there are more moles of gas on one side of the reaction than the other).
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A decrease in radiative equilibrium temperature
Other aspects of the system (such as heat) will change to maintain equilibrium
If the system contain water and gas above it and is closed, no. Only the time to get an equilibrium pressure may shorten
decreases
Yes. If the pressure is increased, even with a noble gas, the reaction equilibrium will shift to alleviate and lower that increased pressure (if there are more moles of gas on one side of the reaction than the other).
Pressure decreases.
presure i increased when more particels hit the side
The pressure will increase if the volume remains the same.
false
Volume decrease.
The pressure of a gas increases with an increase in temperature.