<p>I could understand the principle but i could not explain it on a molecular level for change in pressure and change in temeprature.Why when we increase the pressure of the container,will the equilibrium shift to the side with less molecules??and also for the change in temperature?I would like an explanation on a molecular lever.Thank You</p>
<p>The molecules will have more kinetic energy when you increase the pressure. Hence they will tend to react more, so initially the rate of the forward reaction will increase. That means there will be more products and more molecules at the side where there were less molecules initially. Hence the reaction rate from that side will increase. So eventually the equilibrium will shift to the side with less molecules. The reason is same for higher temperature. The kinetic energy of the molecules increases with higher temperature.</p>