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H2SO4 + Fe3O4 = H2O + FeSO4 + Fe2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + FeO·Fe_2O_3 iron(II, III) oxide ⟶ H_2O water + FeSO_4 duretter + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
H_2SO_4 sulfuric acid + FeO·Fe_2O_3 iron(II, III) oxide ⟶ H_2O water + FeSO_4 duretter + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + FeO·Fe_2O_3 ⟶ H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeO·Fe_2O_3 ⟶ c_3 H_2O + c_4 FeSO_4 + c_5 Fe_2(SO_4)_3·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 4 c_2 = c_3 + 4 c_4 + 12 c_5 S: | c_1 = c_4 + 3 c_5 Fe: | 3 c_2 = c_4 + 2 c_5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + FeO·Fe_2O_3 ⟶ 4 H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: H_2SO_4 + FeO·Fe_2O_3 ⟶ H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 FeO·Fe_2O_3 ⟶ c_3 H_2O + c_4 FeSO_4 + c_5 Fe_2(SO_4)_3·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 4 c_2 = c_3 + 4 c_4 + 12 c_5 S: | c_1 = c_4 + 3 c_5 Fe: | 3 c_2 = c_4 + 2 c_5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + FeO·Fe_2O_3 ⟶ 4 H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O

Structures

+ ⟶ + +
+ ⟶ + +

Names

sulfuric acid + iron(II, III) oxide ⟶ water + duretter + iron(III) sulfate hydrate
sulfuric acid + iron(II, III) oxide ⟶ water + duretter + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + FeO·Fe_2O_3 ⟶ H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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: 4 H_2SO_4 + FeO·Fe_2O_3 ⟶ 4 H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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 H_2SO_4 | 4 | -4 FeO·Fe_2O_3 | 1 | -1 H_2O | 4 | 4 FeSO_4 | 1 | 1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) FeO·Fe_2O_3 | 1 | -1 | ([FeO·Fe2O3])^(-1) H_2O | 4 | 4 | ([H2O])^4 FeSO_4 | 1 | 1 | [FeSO4] Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] 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 = ([H2SO4])^(-4) ([FeO·Fe2O3])^(-1) ([H2O])^4 [FeSO4] [Fe2(SO4)3·xH2O] = (([H2O])^4 [FeSO4] [Fe2(SO4)3·xH2O])/(([H2SO4])^4 [FeO·Fe2O3])
Construct the equilibrium constant, K, expression for: H_2SO_4 + FeO·Fe_2O_3 ⟶ H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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: 4 H_2SO_4 + FeO·Fe_2O_3 ⟶ 4 H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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 H_2SO_4 | 4 | -4 FeO·Fe_2O_3 | 1 | -1 H_2O | 4 | 4 FeSO_4 | 1 | 1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) FeO·Fe_2O_3 | 1 | -1 | ([FeO·Fe2O3])^(-1) H_2O | 4 | 4 | ([H2O])^4 FeSO_4 | 1 | 1 | [FeSO4] Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] 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 = ([H2SO4])^(-4) ([FeO·Fe2O3])^(-1) ([H2O])^4 [FeSO4] [Fe2(SO4)3·xH2O] = (([H2O])^4 [FeSO4] [Fe2(SO4)3·xH2O])/(([H2SO4])^4 [FeO·Fe2O3])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + FeO·Fe_2O_3 ⟶ H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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: 4 H_2SO_4 + FeO·Fe_2O_3 ⟶ 4 H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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 H_2SO_4 | 4 | -4 FeO·Fe_2O_3 | 1 | -1 H_2O | 4 | 4 FeSO_4 | 1 | 1 Fe_2(SO_4)_3·xH_2O | 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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) FeO·Fe_2O_3 | 1 | -1 | -(Δ[FeO·Fe2O3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) FeSO_4 | 1 | 1 | (Δ[FeSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -(Δ[FeO·Fe2O3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[FeSO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + FeO·Fe_2O_3 ⟶ H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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: 4 H_2SO_4 + FeO·Fe_2O_3 ⟶ 4 H_2O + FeSO_4 + Fe_2(SO_4)_3·xH_2O 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 H_2SO_4 | 4 | -4 FeO·Fe_2O_3 | 1 | -1 H_2O | 4 | 4 FeSO_4 | 1 | 1 Fe_2(SO_4)_3·xH_2O | 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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) FeO·Fe_2O_3 | 1 | -1 | -(Δ[FeO·Fe2O3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) FeSO_4 | 1 | 1 | (Δ[FeSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -(Δ[FeO·Fe2O3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[FeSO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | iron(II, III) oxide | water | duretter | iron(III) sulfate hydrate formula | H_2SO_4 | FeO·Fe_2O_3 | H_2O | FeSO_4 | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | Fe_3O_4 | H_2O | FeO_4S | Fe_2O_12S_3 name | sulfuric acid | iron(II, III) oxide | water | duretter | iron(III) sulfate hydrate IUPAC name | sulfuric acid | | water | iron(+2) cation sulfate | diferric trisulfate
| sulfuric acid | iron(II, III) oxide | water | duretter | iron(III) sulfate hydrate formula | H_2SO_4 | FeO·Fe_2O_3 | H_2O | FeSO_4 | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | Fe_3O_4 | H_2O | FeO_4S | Fe_2O_12S_3 name | sulfuric acid | iron(II, III) oxide | water | duretter | iron(III) sulfate hydrate IUPAC name | sulfuric acid | | water | iron(+2) cation sulfate | diferric trisulfate

Substance properties

| sulfuric acid | iron(II, III) oxide | water | duretter | iron(III) sulfate hydrate molar mass | 98.07 g/mol | 231.53 g/mol | 18.015 g/mol | 151.9 g/mol | 399.9 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | | melting point | 10.371 °C | 1538 °C | 0 °C | | boiling point | 279.6 °C | | 99.9839 °C | | density | 1.8305 g/cm^3 | 5 g/cm^3 | 1 g/cm^3 | 2.841 g/cm^3 | solubility in water | very soluble | | | | slightly soluble surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |
| sulfuric acid | iron(II, III) oxide | water | duretter | iron(III) sulfate hydrate molar mass | 98.07 g/mol | 231.53 g/mol | 18.015 g/mol | 151.9 g/mol | 399.9 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | | melting point | 10.371 °C | 1538 °C | 0 °C | | boiling point | 279.6 °C | | 99.9839 °C | | density | 1.8305 g/cm^3 | 5 g/cm^3 | 1 g/cm^3 | 2.841 g/cm^3 | solubility in water | very soluble | | | | slightly soluble surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |

Units

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