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H2SO4 + H2O2 + Fe(SO4) = H2O + Fe2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide + FeSO_4·7H_2O ironate ⟶ H_2O water + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide + FeSO_4·7H_2O ironate ⟶ H_2O water + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + H_2O_2 + FeSO_4·7H_2O ⟶ H_2O + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2O_2 + c_3 FeSO_4·7H_2O ⟶ c_4 H_2O + 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_2 + 14 c_3 = 2 c_4 O: | 4 c_1 + 2 c_2 + 11 c_3 = c_4 + 12 c_5 S: | c_1 + c_3 = 3 c_5 Fe: | c_3 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 16 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + H_2O_2 + 2 FeSO_4·7H_2O ⟶ 16 H_2O + Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: H_2SO_4 + H_2O_2 + FeSO_4·7H_2O ⟶ H_2O + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2O_2 + c_3 FeSO_4·7H_2O ⟶ c_4 H_2O + 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_2 + 14 c_3 = 2 c_4 O: | 4 c_1 + 2 c_2 + 11 c_3 = c_4 + 12 c_5 S: | c_1 + c_3 = 3 c_5 Fe: | c_3 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 16 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + H_2O_2 + 2 FeSO_4·7H_2O ⟶ 16 H_2O + Fe_2(SO_4)_3·xH_2O

Structures

+ + ⟶ +
+ + ⟶ +

Names

sulfuric acid + hydrogen peroxide + ironate ⟶ water + iron(III) sulfate hydrate
sulfuric acid + hydrogen peroxide + ironate ⟶ water + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2O_2 + FeSO_4·7H_2O ⟶ H_2O + 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: H_2SO_4 + H_2O_2 + 2 FeSO_4·7H_2O ⟶ 16 H_2O + 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 | 1 | -1 H_2O_2 | 1 | -1 FeSO_4·7H_2O | 2 | -2 H_2O | 16 | 16 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 | 1 | -1 | ([H2SO4])^(-1) H_2O_2 | 1 | -1 | ([H2O2])^(-1) FeSO_4·7H_2O | 2 | -2 | ([FeSO4·7H2O])^(-2) H_2O | 16 | 16 | ([H2O])^16 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])^(-1) ([H2O2])^(-1) ([FeSO4·7H2O])^(-2) ([H2O])^16 [Fe2(SO4)3·xH2O] = (([H2O])^16 [Fe2(SO4)3·xH2O])/([H2SO4] [H2O2] ([FeSO4·7H2O])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2O_2 + FeSO_4·7H_2O ⟶ H_2O + 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: H_2SO_4 + H_2O_2 + 2 FeSO_4·7H_2O ⟶ 16 H_2O + 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 | 1 | -1 H_2O_2 | 1 | -1 FeSO_4·7H_2O | 2 | -2 H_2O | 16 | 16 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 | 1 | -1 | ([H2SO4])^(-1) H_2O_2 | 1 | -1 | ([H2O2])^(-1) FeSO_4·7H_2O | 2 | -2 | ([FeSO4·7H2O])^(-2) H_2O | 16 | 16 | ([H2O])^16 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])^(-1) ([H2O2])^(-1) ([FeSO4·7H2O])^(-2) ([H2O])^16 [Fe2(SO4)3·xH2O] = (([H2O])^16 [Fe2(SO4)3·xH2O])/([H2SO4] [H2O2] ([FeSO4·7H2O])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + H_2O_2 + FeSO_4·7H_2O ⟶ H_2O + 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: H_2SO_4 + H_2O_2 + 2 FeSO_4·7H_2O ⟶ 16 H_2O + 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 | 1 | -1 H_2O_2 | 1 | -1 FeSO_4·7H_2O | 2 | -2 H_2O | 16 | 16 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) FeSO_4·7H_2O | 2 | -2 | -1/2 (Δ[FeSO4·7H2O])/(Δt) H_2O | 16 | 16 | 1/16 (Δ[H2O])/(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 = -(Δ[H2SO4])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[FeSO4·7H2O])/(Δt) = 1/16 (Δ[H2O])/(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 + H_2O_2 + FeSO_4·7H_2O ⟶ H_2O + 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: H_2SO_4 + H_2O_2 + 2 FeSO_4·7H_2O ⟶ 16 H_2O + 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 | 1 | -1 H_2O_2 | 1 | -1 FeSO_4·7H_2O | 2 | -2 H_2O | 16 | 16 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) FeSO_4·7H_2O | 2 | -2 | -1/2 (Δ[FeSO4·7H2O])/(Δt) H_2O | 16 | 16 | 1/16 (Δ[H2O])/(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 = -(Δ[H2SO4])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[FeSO4·7H2O])/(Δt) = 1/16 (Δ[H2O])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen peroxide | ironate | water | iron(III) sulfate hydrate formula | H_2SO_4 | H_2O_2 | FeSO_4·7H_2O | H_2O | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | H_2O_2 | FeH_14O_11S | H_2O | Fe_2O_12S_3 name | sulfuric acid | hydrogen peroxide | ironate | water | iron(III) sulfate hydrate IUPAC name | sulfuric acid | hydrogen peroxide | iron(+2) cation sulfate heptahydrate | water | diferric trisulfate
| sulfuric acid | hydrogen peroxide | ironate | water | iron(III) sulfate hydrate formula | H_2SO_4 | H_2O_2 | FeSO_4·7H_2O | H_2O | Fe_2(SO_4)_3·xH_2O Hill formula | H_2O_4S | H_2O_2 | FeH_14O_11S | H_2O | Fe_2O_12S_3 name | sulfuric acid | hydrogen peroxide | ironate | water | iron(III) sulfate hydrate IUPAC name | sulfuric acid | hydrogen peroxide | iron(+2) cation sulfate heptahydrate | water | diferric trisulfate

Substance properties

| sulfuric acid | hydrogen peroxide | ironate | water | iron(III) sulfate hydrate molar mass | 98.07 g/mol | 34.014 g/mol | 278.01 g/mol | 18.015 g/mol | 399.9 g/mol phase | liquid (at STP) | liquid (at STP) | | liquid (at STP) | melting point | 10.371 °C | -0.43 °C | | 0 °C | boiling point | 279.6 °C | 150.2 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | 1.44 g/cm^3 | 1.9 g/cm^3 | 1 g/cm^3 | solubility in water | very soluble | miscible | | | slightly soluble surface tension | 0.0735 N/m | 0.0804 N/m | | 0.0728 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | | odorless |
| sulfuric acid | hydrogen peroxide | ironate | water | iron(III) sulfate hydrate molar mass | 98.07 g/mol | 34.014 g/mol | 278.01 g/mol | 18.015 g/mol | 399.9 g/mol phase | liquid (at STP) | liquid (at STP) | | liquid (at STP) | melting point | 10.371 °C | -0.43 °C | | 0 °C | boiling point | 279.6 °C | 150.2 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | 1.44 g/cm^3 | 1.9 g/cm^3 | 1 g/cm^3 | solubility in water | very soluble | miscible | | | slightly soluble surface tension | 0.0735 N/m | 0.0804 N/m | | 0.0728 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | | odorless |

Units

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