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Fe2(SO4)3 + K4[Fe(CN)6] = K2SO4 + Fe4[Fe(CN)6]3

Input interpretation

Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + K4Fe(CN)6 ⟶ K_2SO_4 potassium sulfate + Fe4(Fe(CN)6)3
Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + K4Fe(CN)6 ⟶ K_2SO_4 potassium sulfate + Fe4(Fe(CN)6)3

Balanced equation

Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + K4Fe(CN)6 ⟶ K_2SO_4 + Fe4(Fe(CN)6)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 K4Fe(CN)6 ⟶ c_3 K_2SO_4 + c_4 Fe4(Fe(CN)6)3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, K, C and N: Fe: | 2 c_1 + c_2 = 7 c_4 O: | 12 c_1 = 4 c_3 S: | 3 c_1 = c_3 K: | 4 c_2 = 2 c_3 C: | 6 c_2 = 18 c_4 N: | 6 c_2 = 18 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 6 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Fe_2(SO_4)_3·xH_2O + 3 K4Fe(CN)6 ⟶ 6 K_2SO_4 + Fe4(Fe(CN)6)3
Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + K4Fe(CN)6 ⟶ K_2SO_4 + Fe4(Fe(CN)6)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 K4Fe(CN)6 ⟶ c_3 K_2SO_4 + c_4 Fe4(Fe(CN)6)3 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, K, C and N: Fe: | 2 c_1 + c_2 = 7 c_4 O: | 12 c_1 = 4 c_3 S: | 3 c_1 = c_3 K: | 4 c_2 = 2 c_3 C: | 6 c_2 = 18 c_4 N: | 6 c_2 = 18 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 6 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Fe_2(SO_4)_3·xH_2O + 3 K4Fe(CN)6 ⟶ 6 K_2SO_4 + Fe4(Fe(CN)6)3

Structures

+ K4Fe(CN)6 ⟶ + Fe4(Fe(CN)6)3
+ K4Fe(CN)6 ⟶ + Fe4(Fe(CN)6)3

Names

iron(III) sulfate hydrate + K4Fe(CN)6 ⟶ potassium sulfate + Fe4(Fe(CN)6)3
iron(III) sulfate hydrate + K4Fe(CN)6 ⟶ potassium sulfate + Fe4(Fe(CN)6)3

Equilibrium constant

Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + K4Fe(CN)6 ⟶ K_2SO_4 + Fe4(Fe(CN)6)3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 Fe_2(SO_4)_3·xH_2O + 3 K4Fe(CN)6 ⟶ 6 K_2SO_4 + Fe4(Fe(CN)6)3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i Fe_2(SO_4)_3·xH_2O | 2 | -2 K4Fe(CN)6 | 3 | -3 K_2SO_4 | 6 | 6 Fe4(Fe(CN)6)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe_2(SO_4)_3·xH_2O | 2 | -2 | ([Fe2(SO4)3·xH2O])^(-2) K4Fe(CN)6 | 3 | -3 | ([K4Fe(CN)6])^(-3) K_2SO_4 | 6 | 6 | ([K2SO4])^6 Fe4(Fe(CN)6)3 | 1 | 1 | [Fe4(Fe(CN)6)3] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([Fe2(SO4)3·xH2O])^(-2) ([K4Fe(CN)6])^(-3) ([K2SO4])^6 [Fe4(Fe(CN)6)3] = (([K2SO4])^6 [Fe4(Fe(CN)6)3])/(([Fe2(SO4)3·xH2O])^2 ([K4Fe(CN)6])^3)
Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + K4Fe(CN)6 ⟶ K_2SO_4 + Fe4(Fe(CN)6)3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 Fe_2(SO_4)_3·xH_2O + 3 K4Fe(CN)6 ⟶ 6 K_2SO_4 + Fe4(Fe(CN)6)3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i Fe_2(SO_4)_3·xH_2O | 2 | -2 K4Fe(CN)6 | 3 | -3 K_2SO_4 | 6 | 6 Fe4(Fe(CN)6)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe_2(SO_4)_3·xH_2O | 2 | -2 | ([Fe2(SO4)3·xH2O])^(-2) K4Fe(CN)6 | 3 | -3 | ([K4Fe(CN)6])^(-3) K_2SO_4 | 6 | 6 | ([K2SO4])^6 Fe4(Fe(CN)6)3 | 1 | 1 | [Fe4(Fe(CN)6)3] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([Fe2(SO4)3·xH2O])^(-2) ([K4Fe(CN)6])^(-3) ([K2SO4])^6 [Fe4(Fe(CN)6)3] = (([K2SO4])^6 [Fe4(Fe(CN)6)3])/(([Fe2(SO4)3·xH2O])^2 ([K4Fe(CN)6])^3)

Rate of reaction

Construct the rate of reaction expression for: Fe_2(SO_4)_3·xH_2O + K4Fe(CN)6 ⟶ K_2SO_4 + Fe4(Fe(CN)6)3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 Fe_2(SO_4)_3·xH_2O + 3 K4Fe(CN)6 ⟶ 6 K_2SO_4 + Fe4(Fe(CN)6)3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i Fe_2(SO_4)_3·xH_2O | 2 | -2 K4Fe(CN)6 | 3 | -3 K_2SO_4 | 6 | 6 Fe4(Fe(CN)6)3 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term Fe_2(SO_4)_3·xH_2O | 2 | -2 | -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) K4Fe(CN)6 | 3 | -3 | -1/3 (Δ[K4Fe(CN)6])/(Δt) K_2SO_4 | 6 | 6 | 1/6 (Δ[K2SO4])/(Δt) Fe4(Fe(CN)6)3 | 1 | 1 | (Δ[Fe4(Fe(CN)6)3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) = -1/3 (Δ[K4Fe(CN)6])/(Δt) = 1/6 (Δ[K2SO4])/(Δt) = (Δ[Fe4(Fe(CN)6)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Fe_2(SO_4)_3·xH_2O + K4Fe(CN)6 ⟶ K_2SO_4 + Fe4(Fe(CN)6)3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 Fe_2(SO_4)_3·xH_2O + 3 K4Fe(CN)6 ⟶ 6 K_2SO_4 + Fe4(Fe(CN)6)3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i Fe_2(SO_4)_3·xH_2O | 2 | -2 K4Fe(CN)6 | 3 | -3 K_2SO_4 | 6 | 6 Fe4(Fe(CN)6)3 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term Fe_2(SO_4)_3·xH_2O | 2 | -2 | -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) K4Fe(CN)6 | 3 | -3 | -1/3 (Δ[K4Fe(CN)6])/(Δt) K_2SO_4 | 6 | 6 | 1/6 (Δ[K2SO4])/(Δt) Fe4(Fe(CN)6)3 | 1 | 1 | (Δ[Fe4(Fe(CN)6)3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[Fe2(SO4)3·xH2O])/(Δt) = -1/3 (Δ[K4Fe(CN)6])/(Δt) = 1/6 (Δ[K2SO4])/(Δt) = (Δ[Fe4(Fe(CN)6)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(III) sulfate hydrate | K4Fe(CN)6 | potassium sulfate | Fe4(Fe(CN)6)3 formula | Fe_2(SO_4)_3·xH_2O | K4Fe(CN)6 | K_2SO_4 | Fe4(Fe(CN)6)3 Hill formula | Fe_2O_12S_3 | C6FeK4N6 | K_2O_4S | C18Fe7N18 name | iron(III) sulfate hydrate | | potassium sulfate | IUPAC name | diferric trisulfate | | dipotassium sulfate |
| iron(III) sulfate hydrate | K4Fe(CN)6 | potassium sulfate | Fe4(Fe(CN)6)3 formula | Fe_2(SO_4)_3·xH_2O | K4Fe(CN)6 | K_2SO_4 | Fe4(Fe(CN)6)3 Hill formula | Fe_2O_12S_3 | C6FeK4N6 | K_2O_4S | C18Fe7N18 name | iron(III) sulfate hydrate | | potassium sulfate | IUPAC name | diferric trisulfate | | dipotassium sulfate |

Substance properties

| iron(III) sulfate hydrate | K4Fe(CN)6 | potassium sulfate | Fe4(Fe(CN)6)3 molar mass | 399.9 g/mol | 368.35 g/mol | 174.25 g/mol | 859.24 g/mol solubility in water | slightly soluble | | soluble |
| iron(III) sulfate hydrate | K4Fe(CN)6 | potassium sulfate | Fe4(Fe(CN)6)3 molar mass | 399.9 g/mol | 368.35 g/mol | 174.25 g/mol | 859.24 g/mol solubility in water | slightly soluble | | soluble |

Units

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