Le'chetelliers principle states that when an external factor such as temperature and pressure is added to a system in equilibrium...the disequilibrium will shift so as to annul the effect
Explanation:
To know the cause of increase in pressure in the above equation ...
You should note 2 things
1. the number of moles of all gaseous elements on both side and 2. How change in temperature will affect the equilibrium....
There are 4 moles on the left and 2 on the right ..
making it 4 : 1
so...increase in temperature will shift the equilibrium to the favour the reaction with fewer molecules thereby shifting it right ...the reverse is the case as to decrease in temperature
however; increase in temperature ...if it's an endothermic reaction having a positive sign...tge equilibrium will shift to the right and there will be increase in K....the reverse also is the case as to an exothermic reaction where delta h is negative -ve
Le’Châtlier’s principle states that the equilibrium will shift in order to minimise the effect of the imposed change.
A change in temperature will cause the equilibrium to shift in a particular direction to reduce the effect of the temperature. A change in pressure will cause the equilibrium to shift in a particular direction to reduce the effect of the pressure.
If the reaction is N2(g) + 3H2(g) = 2NH3, increasing the temperature will cause equilibrium to shift to the left. As the forward reaction is an exothermic process, and the backwards reaction is an endothermic process, the excess heat will be absorbed to form N2 and H2. This increases the concentration of N2 and H2
If the reaction is, N2(g) + 3H2(g) = 2NH3, increasing the pressure will cause equilibrium to shift to the right. Increasing pressure means that the side of the equation with the least moles will be favoured and more of it will be produced. Therefore, there will be a higher concentration of NH3
