When solutions of yellow Fe+3(aq) and Fe+3(aq) and colorless SCN (aq) are mixed, a red complex ion forms
Fe^3+(aq) + SCN^- (aq) = Fe(SCN)^2+ (aq)

a) What change would be observed when a solution of Fe+3(aq) is added to this equilibrium
containing an excess of SCN-(aq)?

b) What change to the solution color would be observed when a solution of Ag+ (aq) is added to
equilibrium containing an excess of SCN (aq)? (Hint Agt forms a precipitate with SCN)

c) Explain how these observations are consistent with Le Chatlier's Principle.

Answer and explanantion:

PART A

If you add Fe+3 ions, the shift goes toward products, since there is excess of reactants . So, the solutoin gets more RED . It is consistent, since more reagent will favour more produciton of FeSCN, therefore, the red color must increase

PART B

If you add Ag+ ions, then you will have AgSCN production

SCN- decreases, so the reagents decrease . The reaction stops productino of FeSCN complex, and the complex starts formid reactants , so the color goes more YELLOW .

PART C

This is consistent, since Q = [products] / [reactants] constant must be kept.

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.