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3. When Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6]...
3. When C12(g) is added to aqueous K4[Fe(CN).), [Fe(CN)]*- is oxidized to [Fe(CN).]>- and K:[Fe(CN)] precipitates, as shown below. 2K.[Fe(CN),](aq) +Cl2(g) = 2Ks[Fe(CN)2](3) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C [Fe(CN).J” (aq) + € → [Fe(CN).]" (aq) E = 0.356 V Cl2(g) + 2e → 2Cl(aq) E* = 1.360 V Kup of Kj[Fe(CN).] = 106.5 Answer: b. When 80.0 mL of 1.00 M KCN is added to...
3. When Clz(9) is added to aqueous Ke[Fe(CN).), [Fe(CN).]*- is oxidized to [Fe(CN).jº-and Kz[Fe(CN).] precipitates, as shown below. 2K [Fe(CN)6] (aq) +C12(g) = 2K [Fe(CN).](s) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C: [Fe(CN)6]3-(aq) + [Fe(CN)6]+-(aq) E° = 0.356 V Cl2(g) + 2e + 2Cl(aq) E° = 1.360 V Ksp of K3[Fe(CN)6] = 106.5
Calculate the equilibrium constant K for the reactions at 298 K. a) Br2(g) + 2Cl-(aq) ---> 2Br-(aq) + Cl2(g) b) A Galvanic Cell with the SHE and Fe+2/Fe(s)
1.) 2Cl Cl2(g) K = 3.44 x 105 What happens if the concentrations of Cl is 0.045 M and the concentration of Cl2 is 0.23 M? A) the reaction will proceed to the right B) the reaction will proceed to the left C) The reaction will stay the same D) Not enough information to figure this out. 2.) We have FeCl2. We can put this into a solution of either 0.1 M Fe(NO3)3 or 0.1 M MgCl2. Which one will result...
O KINETICS AND EQUILIBRIUM Using Kf to calculate the equilibrium molarity of a complex For the aqueous [Fe(CN)614 complex K,=1.0 x 1035 at 25 °C. Suppose equal volumes of 0.0090 M Fe(N Dz) solution and 0.98 M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Feion. Round your answer to 2 significant digits. | Ом x 6 ?
3. (2 pts) Which reaction below illustrates ligand substitution? Circle the one correct answer. a) 2 AgNO3 (aq) + CaCl2 (aq) + 2 AgCl (s) + Ca(NO3)2 (aq) b) AgCl (s) + NaCl (aq) → Na[AgCl2] (aq) c) K3[Fe(SCN)6] (aq) + K4(EDTA) (aq) → K[Fe(EDTA)](aq) + 6 KSCN (aq) d) [Fe(H2O).](NO3)3 (aq) → [Fe(H2O)s(OH)](NO3)2 (aq) + HNO3 (aq) e) 2 K4[Fe(CN)6] + Cl2 → 2 K3[Fe(CN)6] + 2 KCI
answ 10. 11, 12 xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Which of the of the following changes in condition will cause the equilibrium to shift to the right? (3 pts) (A) add Fe (B) removeCO ( C M CO (D) raise the temperature . Calculate the equilibrium copcentrations of land lat 700 K in a vessel that contains initial concentration of HI -0.36 M. The equilibrium...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PC13(g) + Cl2(g) = PC15(g) Calculate the equilibrium concentrations of reactant and products when 0.389 moles of PC13 and 0.389 moles of Cl2 are introduced into a 1.00 L vessel at 500 K [PC13] = [Cl] = [PC15] - The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.467 moles of NHACI(S)...
A) , and in Co(NH3)4Cl 2]NO 3, the counter ion is In K 4[Fe(CN) 6], the counter ion is akt:cr b.kt; NO3- C. CN ; cr d. CN ; NO3 e. Fe2+, CO3+ B) How many ions are formed when [CO(NH 3) 5CICI 2 dissolves in water? a. 5 d. 4 e. 2 C) What is the oxidation state of the nickel atom in the Ni(CN) 53 complex ion? a. +1 b.+3 C. +2 d. +4 e. +0 ОООО oooo...
3.(12pts) The reaction Cl(aq) + HS(a) determined DRL S)+(aq) +2 Cl(aq) has the experimentally rate k[Cl2][H2S] Which of the following mechanisms is(are) consistent with the experimental results. Mech I Mech 11, Mech III Cl2 +H2S >H CI CI+HS (slow) CI+ + HS. …>H+ + Cl. + S H2S = HS. + H+ HSCl2 2CI +S+H (fast) (fast equil) (slow) H2S HS+H (fast equil) (fast equil) (slow) 4. (10 pts) Write the equilibrium constant Ke expression for the following 4 KO:(s)...