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Fe2(SO4)3 + BaCl2 = FeCl3 + BaSO4

Input interpretation

Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + BaCl_2 barium chloride ⟶ FeCl_3 iron(III) chloride + BaSO_4 barium sulfate
Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + BaCl_2 barium chloride ⟶ FeCl_3 iron(III) chloride + BaSO_4 barium sulfate

Balanced equation

Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + BaCl_2 ⟶ FeCl_3 + BaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 BaCl_2 ⟶ c_3 FeCl_3 + c_4 BaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, Ba and Cl: Fe: | 2 c_1 = c_3 O: | 12 c_1 = 4 c_4 S: | 3 c_1 = c_4 Ba: | c_2 = c_4 Cl: | 2 c_2 = 3 c_3 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 = 3 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe_2(SO_4)_3·xH_2O + 3 BaCl_2 ⟶ 2 FeCl_3 + 3 BaSO_4
Balance the chemical equation algebraically: Fe_2(SO_4)_3·xH_2O + BaCl_2 ⟶ FeCl_3 + BaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe_2(SO_4)_3·xH_2O + c_2 BaCl_2 ⟶ c_3 FeCl_3 + c_4 BaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S, Ba and Cl: Fe: | 2 c_1 = c_3 O: | 12 c_1 = 4 c_4 S: | 3 c_1 = c_4 Ba: | c_2 = c_4 Cl: | 2 c_2 = 3 c_3 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 = 3 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Fe_2(SO_4)_3·xH_2O + 3 BaCl_2 ⟶ 2 FeCl_3 + 3 BaSO_4

Structures

+ ⟶ +
+ ⟶ +

Names

iron(III) sulfate hydrate + barium chloride ⟶ iron(III) chloride + barium sulfate
iron(III) sulfate hydrate + barium chloride ⟶ iron(III) chloride + barium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + BaCl_2 ⟶ FeCl_3 + BaSO_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 + 3 BaCl_2 ⟶ 2 FeCl_3 + 3 BaSO_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 BaCl_2 | 3 | -3 FeCl_3 | 2 | 2 BaSO_4 | 3 | 3 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) BaCl_2 | 3 | -3 | ([BaCl2])^(-3) FeCl_3 | 2 | 2 | ([FeCl3])^2 BaSO_4 | 3 | 3 | ([BaSO4])^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])^(-1) ([BaCl2])^(-3) ([FeCl3])^2 ([BaSO4])^3 = (([FeCl3])^2 ([BaSO4])^3)/([Fe2(SO4)3·xH2O] ([BaCl2])^3)
Construct the equilibrium constant, K, expression for: Fe_2(SO_4)_3·xH_2O + BaCl_2 ⟶ FeCl_3 + BaSO_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 + 3 BaCl_2 ⟶ 2 FeCl_3 + 3 BaSO_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 BaCl_2 | 3 | -3 FeCl_3 | 2 | 2 BaSO_4 | 3 | 3 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) BaCl_2 | 3 | -3 | ([BaCl2])^(-3) FeCl_3 | 2 | 2 | ([FeCl3])^2 BaSO_4 | 3 | 3 | ([BaSO4])^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])^(-1) ([BaCl2])^(-3) ([FeCl3])^2 ([BaSO4])^3 = (([FeCl3])^2 ([BaSO4])^3)/([Fe2(SO4)3·xH2O] ([BaCl2])^3)

Rate of reaction

Construct the rate of reaction expression for: Fe_2(SO_4)_3·xH_2O + BaCl_2 ⟶ FeCl_3 + BaSO_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 + 3 BaCl_2 ⟶ 2 FeCl_3 + 3 BaSO_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 BaCl_2 | 3 | -3 FeCl_3 | 2 | 2 BaSO_4 | 3 | 3 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) BaCl_2 | 3 | -3 | -1/3 (Δ[BaCl2])/(Δt) FeCl_3 | 2 | 2 | 1/2 (Δ[FeCl3])/(Δt) BaSO_4 | 3 | 3 | 1/3 (Δ[BaSO4])/(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) = -1/3 (Δ[BaCl2])/(Δt) = 1/2 (Δ[FeCl3])/(Δt) = 1/3 (Δ[BaSO4])/(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 + BaCl_2 ⟶ FeCl_3 + BaSO_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 + 3 BaCl_2 ⟶ 2 FeCl_3 + 3 BaSO_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 BaCl_2 | 3 | -3 FeCl_3 | 2 | 2 BaSO_4 | 3 | 3 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) BaCl_2 | 3 | -3 | -1/3 (Δ[BaCl2])/(Δt) FeCl_3 | 2 | 2 | 1/2 (Δ[FeCl3])/(Δt) BaSO_4 | 3 | 3 | 1/3 (Δ[BaSO4])/(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) = -1/3 (Δ[BaCl2])/(Δt) = 1/2 (Δ[FeCl3])/(Δt) = 1/3 (Δ[BaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| iron(III) sulfate hydrate | barium chloride | iron(III) chloride | barium sulfate formula | Fe_2(SO_4)_3·xH_2O | BaCl_2 | FeCl_3 | BaSO_4 Hill formula | Fe_2O_12S_3 | BaCl_2 | Cl_3Fe | BaO_4S name | iron(III) sulfate hydrate | barium chloride | iron(III) chloride | barium sulfate IUPAC name | diferric trisulfate | barium(+2) cation dichloride | trichloroiron | barium(+2) cation sulfate
| iron(III) sulfate hydrate | barium chloride | iron(III) chloride | barium sulfate formula | Fe_2(SO_4)_3·xH_2O | BaCl_2 | FeCl_3 | BaSO_4 Hill formula | Fe_2O_12S_3 | BaCl_2 | Cl_3Fe | BaO_4S name | iron(III) sulfate hydrate | barium chloride | iron(III) chloride | barium sulfate IUPAC name | diferric trisulfate | barium(+2) cation dichloride | trichloroiron | barium(+2) cation sulfate

Substance properties

| iron(III) sulfate hydrate | barium chloride | iron(III) chloride | barium sulfate molar mass | 399.9 g/mol | 208.2 g/mol | 162.2 g/mol | 233.38 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 963 °C | 304 °C | 1345 °C density | | 3.856 g/cm^3 | | 4.5 g/cm^3 solubility in water | slightly soluble | | | insoluble odor | | odorless | |
| iron(III) sulfate hydrate | barium chloride | iron(III) chloride | barium sulfate molar mass | 399.9 g/mol | 208.2 g/mol | 162.2 g/mol | 233.38 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 963 °C | 304 °C | 1345 °C density | | 3.856 g/cm^3 | | 4.5 g/cm^3 solubility in water | slightly soluble | | | insoluble odor | | odorless | |

Units

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