Balance the equations.
Fe3+(aq) + SCN–(aq) <--> FeSCN2+
Ag+(aq) + SCN–(aq) <--> Ag(SCN)4 ^3-
FeSCN2+(aq) + Ag+(aq) <--> Ag(SCN)43- + Fe3+(aq)
Use Le Chatelier’s principle to explain the different colors and how they relate to the disturbance of the equilibrium.
To balance any equation it is necessary that total charge on reactant side and total charge on product side should be same (with sign)
Fe3+(aq) + SCN_ (aq) -------> Fe(SCN)^2+ (It is already balanced as reactant side has +3-1=+2 which is same in product side
Ag+(aq) + 4SCN_(aq) ----------> Ag(SCN)4 ^3- (here we multiply the thiocyanate with 4 to get the charge balanced)
4Fe(SCN)^2+(aq) + Ag+(aq) ---------> Ag(SCN)4 ^3- + 4Fe3+(aq) (here we multiply iron(II) thiocyanate with 4 and iron(III) with 4 to balance the equation)
In the reaction as the concentration of silver ion or iron(II) thiocyanate concentration was decreased, then the to undo the effect equilibrium shifts backward giving blood red color due to iron(II) thiocyanate and vice versa.Similarly if the concentration of Fe3+ was increased it will shift the reaction toward reactant side giving more intensified solution.
Balance the equations. Fe3+(aq) + SCN–(aq) <--> FeSCN2+ Ag+(aq) + SCN–(aq) <--> Ag(SCN)4 ^3- FeSCN2+(aq) +...
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-] = 1.239; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.454 M. What is the numerical value of KC for this equilibrium? KC = __________________ 2) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.370; [SCN-] = 0.777; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.285 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =...
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.2×10−4 M . At equilibrium, [FeSCN2+]= 1.8×10−4 M . Calculate the value of the equilibrium constant (Kc)(Kc). Express your answer using two significant figures.
Consider the reaction represented by the equation: Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq) What is the equilibrium concentration of FeSCN2+ (aq) if a solution is prepared that is initially 6.00 M Fe3+ (aq) and 6.00 M SCN− (aq)? if k was determined to be 0.333
Calculate the equilibrium constant for the reaction Fe3+ (aq0 + SCN (aq)→ FeSCN2+ (aq) given that the mixture of 5 ml of.00359 M SCN- and 5 ML of .00200 M Fe3+ solutions yield 1.68 x 10A- 4 M FeSCN2+ at a given temperature. a.) 23 . B.) 93 d. 8.06 x 10A-3 c.) 124
2. The reaction Fe3+ (aq) + SCN (aq) → FeSCN2+ (aq) produces a dark red color resulting from the formation of FeSCN2+. a. How does the color change if you add more SCN to a solution at equilibrium? (lighter or darker) b. How does the color change if you remove Fe3+ by reacting it with fluoride ions? c. If a reaction proceeds forward when you heat it, and reverse when you cool it, the reaction is [endothermic exothermic).
* PLEASE WRITE OUT ANSWER STEP BY STEP! CONSIDER THE FOLLOWING REACTION: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.2×10−4 M. At equilibrium, [FeSCN2+] = 1.6×10−4 M . PART A: Calculate the value of the equilibrium constant (Kc): [Express your answer using two significant figures] KC = _____________________________
My question is #2 for the reaction Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq). The goal is to predict the color change (darker or lighter) for test tubes 2-8. I have attached the supplemental sheets given to help with the problem. The test tubes 2-8 are being manipulated either by temperature or things being added which can be seen by one of the pictures. 2. For reaction "UCTIONS are increased by the same amount. Fe3+ (aq) + SCN (aq) $...
At a certain temperature, K = 8.60 x 10^-4. for the reaction FeSCN2+(aq) ⇄ Fe3+(aq) + SCN-(aq) Calculate the concentrations of Fe3+, SCN-, and FeSCN2+ in a solution that is initially 2.0 M FeSCN2+.
Part 1 The Balanced Equilibrium Equations: Reactant(s) Product(s) Fe3+(aq) + _SCN (aq) Ag (aq) + _SCN (aq) [FeSCN]*(aq) +_ Ag+ (aq) [Ag(SCN)4] (aq) +___Fe3+ (aq) Cu'*(aq) + H2O(1) Cu²+ (aq) +_NH3(aq) [Cu(H20)4]2+(aq) + _NH3(aq) [Cu(NH3)4]?*(aq) +_H20(1) _ HNO3(aq) + _NH3(aq) __NH4OH(aq) All Co2+(aq) + _H2O(1) Co2+(aq) +_ Cl(aq) _[Co(H2O).)+(aq) +_ Cl(aq) - [CoCal” (aq) + H2O) *Side reaction
2. The stock solution at equilibrium used in test tube # 4 contains Fe3 (aq), SCN-(aq) and [FESCNP2 (aq). When NaOH was added to test tube #4 a shift in the equilibrium was observed. What chemical species in the stock solution reacted with NAOH? Write the balanced chemical reaction associated with the change observed from the addition of NaOH to test tube #4? Explain in terms of LeChatelier's Principle the observed results from the addition of 0.1 M KSCN to...