Consider a solution containing A, B, and C, reacting according to the following
ID: 775822 • Letter: C
Question
Consider a solution containing A, B, and C, reacting according to the following reversible reaction. The color of the species are indicated:
A (aq) [blue] + 2B (aq) [colorless] <--> C (aq) [colorless]
1. When you add B to the solution, the color changes to <lighter blue>. Is it because since the reaction will shift to the right to re-establish equalibrium, more A will be used up, thus making the blue lighter?
2.The reaction C + D <--> E has a large K. What happens to the concentration [A] when D is added to the solution. The answer is it will decrease but I don't understand why. At first I thought it would remain the same because D is not part of the reaction. Do we assume C and D behaves similarly in this case?
Thank you!
Explanation / Answer
a. If more reactant is added, the equation will shift to the right in order to make more product (which will increase the products)
b. If the temperature is decreased, the reaction will shift to the right to create more heat if it is exothermic (which will increase the product), and to the left if it is endothermic (which will decrease the products)
c. If the pressure is decreased, it will shift in the direction where there are more moles of gas present, because it can now take up more space. If the products have more moles of gas, the products will increase, and vise versa