Postlabn Turn in your laboratory notebook pages and answer the following questio

Question

Postlabn Turn in your laboratory notebook pages and answer the following questions. 1) Consider your investigation of Le Chather's principle from this lab and the following Which way will the A B C D A 42 kJ/mol products) Dis added equilibrium shift (toward reactants or toward to the b. A catalyst is added to the system c. B is added to the system d. C is removed from the system products e. The reaction is cooled down B actants 2) Part I. In the equilibrium Fes (aqoyeuow scN (aqockar v Fe(scN)? red, why did the red color become darker when either Fe3 or SCN- was added? 3) Part II. In the equilibrium Niz (a 6NH3(aq)dear a Ni(NH3)62 blue/violet, why did the color change when HCl was added to the equilibrium solution? The Color Chenges because

Explanation / Answer

Q1.

the reaction is endothermic, since dH is positive, and has equal amount of moles in left/right sides

so

a)

if we add products, then, more reactants will be produced to counterbalance equilibrium change

b)

addition of catalyst will NEVER shift equilibrium, since it only increases rate of reaction, not equilibrium ratio

c)

IF we add reactants, we will favour more product formation

d)

removing a product will make a shift toward more product formation

e)

if we cool down the reaction, it will not proceed toward products, since it is endothermic, so it requires heat to form products. Reactants will increase

2)

when we add Fe+3 and SCN- in equilibrium, we favour MORE formation of the complex Fe(SCN)+2, therefore, more RED color iwll be seen

Q3.

When we add HCl, a strong acid, it will react with ammonia, NH3 a weak base

so

the reactants decrease, so the blue/violet color decreases as Ni+2 green incrases

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