Before beginning laboratory, you should be following questions. Briefly state le
ID: 485898 • Letter: B
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Before beginning laboratory, you should be following questions. Briefly state lessthanorequalto Chatelier's principle. Consider the following equilibrium: Baso_4 (s) right lift arrow B_a^2+ (aq) + SO_4^2- (aq); delta H > 0 In which direction will the equilibrium shift if H_2SO_4 is added? Why? Bacl_2 is added? Why? NaCl is added? Why? Heat is added? Why? Consider the following equilibrium for nitrous acid, HNO_2 a weak acid: HNO_2 (aq) + H_2O(t) right lift arrow H_3O^+(aq) + NO_2^-(aq) In which direction will the equilibrium shift if NaNO_2 is added? NaNO_2 is added?Explanation / Answer
Le chatlier principle states that addition of a species in a reaction will tend to shift the equilibrium but the reaction which will reduce the added species will be favoured and hence leading to reducing the concentration of added species.
Changing the concentration of a chemical will shift the equilibrium to the side that would reduce that change in concentration. The chemical system will attempt to partially oppose the change affected to the original state of equilibrium. In turn, the rate of reaction, extent, and yield of products will be altered corresponding to the impact on the system.
This can be illustrated by the equilibrium of ammonia formation
N2 + 3 H2 2 NH3
Suppose we were to increase the concentration of N2 in the system. Using Le Chatelier's principle, we can predict that the amount of methanol will increase, decreasing the total change in N2 . If we are to add a species to the overall reaction, the reaction will favor the side opposing the addition of the species. Likewise, the subtraction of a species would cause the reaction to "fill the gap" and favor the side where the species was reduced. This observation is supported by the collision theory. As the concentration of N2 is increased, the frequency of successful collisions of that reactant would increase also, allowing for an increase in forward reaction, and generation of the product. Even if the desired product is not thermodynamically favored, the end-product can be obtained if it is continuously removed from the solution.
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