Fe(CN)63- has a Kd of 1 x10-42. Write the equation for the dissociation of the complex...
Fe(CN)63- has a Kd of 1 x10-42.
Write the equation for the dissociation of the complex ion.
Would you expect the reaction mixture to be mostly reactants or
products?
Homework Answers
As Kd is very very small .so
reaction is mostly reactants
Add Answer to:
Fe(CN)63- has a Kd of 1 x10-42.
Write the equation for the dissociation of the complex...
Ni(NH3)62+ has a Kf of 1.2*109. Write the reaction equation for the formation of the complex...
Ni(NH3)62+ has a Kf of 1.2*109. Write the reaction equation for the formation of the complex ion and the equilibrium constant of the formation expression. Would the reaction mixture be mostly be complex ions or simple ions? (I don’t really understand how to answer the last question)
Write down the reduction reaction between Fe(CN)63- and Fe(CN)64-; find the standard electrode potential of this...
Write down the reduction reaction between Fe(CN)63- and Fe(CN)64-; find the standard electrode potential of this half reaction. Calculate the ionic strength of 0.1 KCl and 0.1 M Na2SO4, respectively.
Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a...
Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a formation constant of 1.438x1035 . This complex ion has an intense blue color in solution . a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN-1 (aq) solution, what is the concentration of CN-1 (aq) still in solution when the reaction reaches equilibrium? b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II) ion, [Cu(CN)4] -2 (aq), with a...
Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a...
Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a formation constant of 1.438x1035 . This complex ion has an intense blue color in solution . a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN-1 (aq) solution, what is the concentration of CN-1 (aq) still in solution when the reaction reaches equilibrium? b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II) ion, [Cu(CN)4] -2 (aq), with a...
3. Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN).]*(aq), with a formation...
3. Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN).]*(aq), with a formation constant of 1.438x10's. This complex ion has an intense blue color in solution. a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN'(aq) solution, what is the concentration of CN'(aq) still in solution when the reaction reaches equilibrium? b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II)ion, [Cu(CN).] (aq), with a formation constant of 1.028x10”. This complex ion...
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 Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6] precipitates, as shown below. 2K [Fe(CN).] (aq) + Cl2(g) = 2K3[Fe(CN).J(8) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant (10 pts) At 25°C: [Fe(CN).]" (aq) + e[Fe(CN).]" (aq) E° = 0.356 V Cl2(9) + 2e → 2Cl(aq) E° = 1.360 V Ksp of K3 [Fe(CN)6] = 106.5 b. When 80.0 mL of 1.00 M KCN is...
3. When C12(g) is added to aqueous K4[Fe(CN).), [Fe(CN)]*- is oxidized to [Fe(CN).]>- and K:[Fe(CN)] precipitates,...
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...
17.61 Write the chemical equation for the formation of the Cu(CN)2 ion. Then write the K Cusunt 2 CNas expression....
17.61 Write the chemical equation for the formation of the Cu(CN)2 ion. Then write the K Cusunt 2 CNas expression. Culr 17.62 Write the chemical equation for the formation of the Fe(CN)63 ion. Then write the K expression.
just 12 KEF CAND 372 C) de law is: a) Rate = k[Fe(CN)63-1*[I][Fe(CN)64 1°[12] Rate =...
just 12
KEF CAND 372 C) de law is: a) Rate = k[Fe(CN)63-1*[I][Fe(CN)64 1°[12] Rate = k[Fe(CN).-1*[1][Fe(CN). [12] Rate = k[Fe(CN).-)]*[1] d) Rate = k[Fe(CN).-1[15] Rate = k[Fe(CN)63-1[1] [Fe(CN).-) Tabulated below are initial rate data for the reaction: 2Fe(CN).- + 21 2Fe(CN).-- + 12 12. [I do 0.01 0.02 0.02 0.02 0.02 [Fe(CN)64-) 0.01 0.01 0.01 3 [12] 0.01 0.01 0.01 0.01 0.02 Rate (M/s) 1x 10-5 2x 10-5 8 x 10-5 - 8 x 10-5 8 x 10-5 0.02...
The octahedral complex ion [FeCl6]3- has more unpaired spins than the octahedral complex ion [Fe(CN)6]3-. How...
The octahedral complex ion [FeCl6]3- has more unpaired spins than the octahedral complex ion [Fe(CN)6]3-. How many unpaired electrons are present in each species? Compare the Δo values for these complexes. Complex ion # Unpaired electrons Relative Δo [FeCl6]3- _________largersmaller [Fe(CN)6]3- _________largersmaller
3. Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN).]*(aq), with a formation constant of 1.438x10's. This complex ion has an intense blue color in solution. a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN'(aq) solution, what is the concentration of CN'(aq) still in solution when the reaction reaches equilibrium? b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II)ion, [Cu(CN).] (aq), with a formation constant of 1.028x10”. This complex ion...
3. When Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6] precipitates, as shown below. 2K [Fe(CN).] (aq) + Cl2(g) = 2K3[Fe(CN).J(8) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant (10 pts) At 25°C: [Fe(CN).]" (aq) + e[Fe(CN).]" (aq) E° = 0.356 V Cl2(9) + 2e → 2Cl(aq) E° = 1.360 V Ksp of K3 [Fe(CN)6] = 106.5 b. When 80.0 mL of 1.00 M KCN is...
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...
17.61 Write the chemical equation for the formation of the Cu(CN)2 ion. Then write the K Cusunt 2 CNas expression. Culr 17.62 Write the chemical equation for the formation of the Fe(CN)63 ion. Then write the K expression.
just 12
KEF CAND 372 C) de law is: a) Rate = k[Fe(CN)63-1*[I][Fe(CN)64 1°[12] Rate = k[Fe(CN).-1*[1][Fe(CN). [12] Rate = k[Fe(CN).-)]*[1] d) Rate = k[Fe(CN).-1[15] Rate = k[Fe(CN)63-1[1] [Fe(CN).-) Tabulated below are initial rate data for the reaction: 2Fe(CN).- + 21 2Fe(CN).-- + 12 12. [I do 0.01 0.02 0.02 0.02 0.02 [Fe(CN)64-) 0.01 0.01 0.01 3 [12] 0.01 0.01 0.01 0.01 0.02 Rate (M/s) 1x 10-5 2x 10-5 8 x 10-5 - 8 x 10-5 8 x 10-5 0.02...
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