Question

Describe Le Châtelier’s principle, and give an example of an equilibrium shift that might occur to a system.

Answer 1

If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

Answer 2

According to Le Chatelier, the position of equilibrium will move in such a way as to counteract the change. That means that the position of equilibrium will move so that the concentration of A decreases again - by reacting it with B and turning it into C + D. The position of equilibrium moves to the right.

This is a useful way of converting the maximum possible amount of B into C and D. You might use it if, for example, B was a relatively expensive material whereas A was cheap and plentiful.

Answer 3

so like adding water to a soap bottle when you are running low and to lazy to go to the store?

Answer 4

According to Le Chatelier, the position of equilibrium will move so that the concentration of A increases again. That means that more C and D will react to replace the A that has been removed. The position of equilibrium moves to the left.

This is esssentially what happens if you remove one of the products of the reaction as soon as it is formed. If, for example, you removed C as soon as it was formed, the position of equilibrium would move to the right to replace it. If you kept on removing it, the equilibrium position would keep on moving rightwards - turning this into a one-way reaction

Answer 5

YES

Answer 6

The effect of changing the temperature in the equilibrium can be made clear by incorporating heat as either a reactant or a product. When the reaction is exothermic (ΔH is negative, puts energy out), we include heat as a product, and, when the reaction is endothermic (ΔH is positive, takes energy in), we include it as a reactant. Hence, we can determine whether increasing or decreasing the temperature would favour the forward or reverse reaction by applying the same principle as with concentration changes.

Take, for example, the reaction of nitrogen gas with hydrogen gas. This is a reversible reaction, in which the two gases react to form ammonia:

N2 + 3 H2 ⇌ 2 NH3 ΔH = -92 kJ mol-1

The product contains heat:

N2 + 3 H2 ⇌ 2 NH3 + 92kJ

This is an exothermic reaction (hence the minus sign) when producing ammonia. If we were to lower the temperature, the equilibrium would shift to produce more heat. Since making ammonia is exothermic, this would favour the production of more ammonia. In practice, in the Haber process, the temperature is set at a compromise value, so ammonia is made quickly, even though less would be present at equilibrium.

Answer 7

So would this be an appropriate answer to this:
Le Châtelier’ principle, also know as “the Law of Equilibrium”, states that if you have two substances and one is in higher concentration than the other. The one with the higher concentration with mix with the one of lesser concentration.
A+2B = C+D

Answer 8

no.

Answer 9

yeah it is law of equilibrium but u to practise more examples they r different

Answer 10

If a chemical reaciton is at equilibrium and experiences a change such as pressure, temperature, or concentration of products or reactants the equilibrium will shift in the direction to accommodate the change

Answer 11

http://chemwiki.ucdavis.edu/Physical_Chemistry/Chemical_Equilibrium/Le_Chatelier%27s_Principle
this can help u

Answer 12

Thank you. I was starting to stress. I'm gonna go for a few i'll be right back.