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Fe2(SO4)3 + K3PO4 = K2SO4 + FePO4

Input interpretation

Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + K3PO4 ⟶ K_2SO_4 potassium sulfate + FePO_4 iron(III) phosphate
Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + K3PO4 ⟶ K_2SO_4 potassium sulfate + FePO_4 iron(III) phosphate

Balanced equation

Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + K3PO4 ⟶ K_2SO_4 + FePO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 K3PO4 ⟶ c_3 K_2SO_4 + c_4 FePO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, K and P: Fe: | 2 c_1 = c_4 O: | 12 c_1 + 4 c_2 = 4 c_3 + 4 c_4 S: | 3 c_1 = c_3 K: | 3 c_2 = 2 c_3 P: | c_2 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe_2(SO_4)_3·xH_2O + 2 K3PO4 ⟶ 3 K_2SO_4 + 2 FePO_4
Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + K3PO4 ⟶ K_2SO_4 + FePO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 K3PO4 ⟶ c_3 K_2SO_4 + c_4 FePO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, K and P: Fe: | 2 c_1 = c_4 O: | 12 c_1 + 4 c_2 = 4 c_3 + 4 c_4 S: | 3 c_1 = c_3 K: | 3 c_2 = 2 c_3 P: | c_2 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe_2(SO_4)_3·xH_2O + 2 K3PO4 ⟶ 3 K_2SO_4 + 2 FePO_4

Structures

+ K3PO4 ⟶ +
+ K3PO4 ⟶ +

Names

iron(III) sulfate hydrate + K3PO4 ⟶ potassium sulfate + iron(III) phosphate
iron(III) sulfate hydrate + K3PO4 ⟶ potassium sulfate + iron(III) phosphate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + K3PO4 ⟶ K_2SO_4 + FePO_4 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: Fe_2(SO_4)_3·xH_2O + 2 K3PO4 ⟶ 3 K_2SO_4 + 2 FePO_4 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 | 1 | -1 K3PO4 | 2 | -2 K_2SO_4 | 3 | 3 FePO_4 | 2 | 2 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 | 1 | -1 | ([Fe2(SO4)3·xH2O])^(-1) K3PO4 | 2 | -2 | ([K3PO4])^(-2) K_2SO_4 | 3 | 3 | ([K2SO4])^3 FePO_4 | 2 | 2 | ([FePO4])^2 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])^(-1) ([K3PO4])^(-2) ([K2SO4])^3 ([FePO4])^2 = (([K2SO4])^3 ([FePO4])^2)/([Fe2(SO4)3·xH2O] ([K3PO4])^2)
Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + K3PO4 ⟶ K_2SO_4 + FePO_4 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: Fe_2(SO_4)_3·xH_2O + 2 K3PO4 ⟶ 3 K_2SO_4 + 2 FePO_4 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 | 1 | -1 K3PO4 | 2 | -2 K_2SO_4 | 3 | 3 FePO_4 | 2 | 2 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 | 1 | -1 | ([Fe2(SO4)3·xH2O])^(-1) K3PO4 | 2 | -2 | ([K3PO4])^(-2) K_2SO_4 | 3 | 3 | ([K2SO4])^3 FePO_4 | 2 | 2 | ([FePO4])^2 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])^(-1) ([K3PO4])^(-2) ([K2SO4])^3 ([FePO4])^2 = (([K2SO4])^3 ([FePO4])^2)/([Fe2(SO4)3·xH2O] ([K3PO4])^2)

Rate of reaction

Construct the rate of reaction expression for: Fe_2(SO_4)_3·xH_2O + K3PO4 ⟶ K_2SO_4 + FePO_4 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: Fe_2(SO_4)_3·xH_2O + 2 K3PO4 ⟶ 3 K_2SO_4 + 2 FePO_4 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 | 1 | -1 K3PO4 | 2 | -2 K_2SO_4 | 3 | 3 FePO_4 | 2 | 2 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 | 1 | -1 | -(Δ[Fe2(SO4)3·xH2O])/(Δt) K3PO4 | 2 | -2 | -1/2 (Δ[K3PO4])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) FePO_4 | 2 | 2 | 1/2 (Δ[FePO4])/(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 = -(Δ[Fe2(SO4)3·xH2O])/(Δt) = -1/2 (Δ[K3PO4])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/2 (Δ[FePO4])/(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 + K3PO4 ⟶ K_2SO_4 + FePO_4 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: Fe_2(SO_4)_3·xH_2O + 2 K3PO4 ⟶ 3 K_2SO_4 + 2 FePO_4 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 | 1 | -1 K3PO4 | 2 | -2 K_2SO_4 | 3 | 3 FePO_4 | 2 | 2 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 | 1 | -1 | -(Δ[Fe2(SO4)3·xH2O])/(Δt) K3PO4 | 2 | -2 | -1/2 (Δ[K3PO4])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) FePO_4 | 2 | 2 | 1/2 (Δ[FePO4])/(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 = -(Δ[Fe2(SO4)3·xH2O])/(Δt) = -1/2 (Δ[K3PO4])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/2 (Δ[FePO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(III) sulfate hydrate | K3PO4 | potassium sulfate | iron(III) phosphate formula | Fe_2(SO_4)_3·xH_2O | K3PO4 | K_2SO_4 | FePO_4 Hill formula | Fe_2O_12S_3 | K3O4P | K_2O_4S | FeO_4P name | iron(III) sulfate hydrate | | potassium sulfate | iron(III) phosphate IUPAC name | diferric trisulfate | | dipotassium sulfate | iron(+3) cation phosphate
| iron(III) sulfate hydrate | K3PO4 | potassium sulfate | iron(III) phosphate formula | Fe_2(SO_4)_3·xH_2O | K3PO4 | K_2SO_4 | FePO_4 Hill formula | Fe_2O_12S_3 | K3O4P | K_2O_4S | FeO_4P name | iron(III) sulfate hydrate | | potassium sulfate | iron(III) phosphate IUPAC name | diferric trisulfate | | dipotassium sulfate | iron(+3) cation phosphate

Substance properties

| iron(III) sulfate hydrate | K3PO4 | potassium sulfate | iron(III) phosphate molar mass | 399.9 g/mol | 212.26 g/mol | 174.25 g/mol | 150.81 g/mol density | | | | 2.87 g/cm^3 solubility in water | slightly soluble | | soluble |
| iron(III) sulfate hydrate | K3PO4 | potassium sulfate | iron(III) phosphate molar mass | 399.9 g/mol | 212.26 g/mol | 174.25 g/mol | 150.81 g/mol density | | | | 2.87 g/cm^3 solubility in water | slightly soluble | | soluble |

Units

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