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KOH + H2O2 + FeSO4 = K2SO4 + Fe(OH)3

Input interpretation

KOH potassium hydroxide + H_2O_2 hydrogen peroxide + FeSO_4 duretter ⟶ K_2SO_4 potassium sulfate + Fe(OH)_3 iron(III) hydroxide
KOH potassium hydroxide + H_2O_2 hydrogen peroxide + FeSO_4 duretter ⟶ K_2SO_4 potassium sulfate + Fe(OH)_3 iron(III) hydroxide

Balanced equation

Balance the chemical equation algebraically: KOH + H_2O_2 + FeSO_4 ⟶ K_2SO_4 + Fe(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_2O_2 + c_3 FeSO_4 ⟶ c_4 K_2SO_4 + c_5 Fe(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Fe and S: H: | c_1 + 2 c_2 = 3 c_5 K: | c_1 = 2 c_4 O: | c_1 + 2 c_2 + 4 c_3 = 4 c_4 + 3 c_5 Fe: | c_3 = c_5 S: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 KOH + H_2O_2 + 2 FeSO_4 ⟶ 2 K_2SO_4 + 2 Fe(OH)_3
Balance the chemical equation algebraically: KOH + H_2O_2 + FeSO_4 ⟶ K_2SO_4 + Fe(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_2O_2 + c_3 FeSO_4 ⟶ c_4 K_2SO_4 + c_5 Fe(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Fe and S: H: | c_1 + 2 c_2 = 3 c_5 K: | c_1 = 2 c_4 O: | c_1 + 2 c_2 + 4 c_3 = 4 c_4 + 3 c_5 Fe: | c_3 = c_5 S: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 KOH + H_2O_2 + 2 FeSO_4 ⟶ 2 K_2SO_4 + 2 Fe(OH)_3

Structures

+ + ⟶ +
+ + ⟶ +

Names

potassium hydroxide + hydrogen peroxide + duretter ⟶ potassium sulfate + iron(III) hydroxide
potassium hydroxide + hydrogen peroxide + duretter ⟶ potassium sulfate + iron(III) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + H_2O_2 + FeSO_4 ⟶ K_2SO_4 + Fe(OH)_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: 4 KOH + H_2O_2 + 2 FeSO_4 ⟶ 2 K_2SO_4 + 2 Fe(OH)_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 KOH | 4 | -4 H_2O_2 | 1 | -1 FeSO_4 | 2 | -2 K_2SO_4 | 2 | 2 Fe(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 4 | -4 | ([KOH])^(-4) H_2O_2 | 1 | -1 | ([H2O2])^(-1) FeSO_4 | 2 | -2 | ([FeSO4])^(-2) K_2SO_4 | 2 | 2 | ([K2SO4])^2 Fe(OH)_3 | 2 | 2 | ([Fe(OH)3])^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 = ([KOH])^(-4) ([H2O2])^(-1) ([FeSO4])^(-2) ([K2SO4])^2 ([Fe(OH)3])^2 = (([K2SO4])^2 ([Fe(OH)3])^2)/(([KOH])^4 [H2O2] ([FeSO4])^2)
Construct the equilibrium constant, K, expression for: KOH + H_2O_2 + FeSO_4 ⟶ K_2SO_4 + Fe(OH)_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: 4 KOH + H_2O_2 + 2 FeSO_4 ⟶ 2 K_2SO_4 + 2 Fe(OH)_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 KOH | 4 | -4 H_2O_2 | 1 | -1 FeSO_4 | 2 | -2 K_2SO_4 | 2 | 2 Fe(OH)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 4 | -4 | ([KOH])^(-4) H_2O_2 | 1 | -1 | ([H2O2])^(-1) FeSO_4 | 2 | -2 | ([FeSO4])^(-2) K_2SO_4 | 2 | 2 | ([K2SO4])^2 Fe(OH)_3 | 2 | 2 | ([Fe(OH)3])^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 = ([KOH])^(-4) ([H2O2])^(-1) ([FeSO4])^(-2) ([K2SO4])^2 ([Fe(OH)3])^2 = (([K2SO4])^2 ([Fe(OH)3])^2)/(([KOH])^4 [H2O2] ([FeSO4])^2)

Rate of reaction

Construct the rate of reaction expression for: KOH + H_2O_2 + FeSO_4 ⟶ K_2SO_4 + Fe(OH)_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: 4 KOH + H_2O_2 + 2 FeSO_4 ⟶ 2 K_2SO_4 + 2 Fe(OH)_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 KOH | 4 | -4 H_2O_2 | 1 | -1 FeSO_4 | 2 | -2 K_2SO_4 | 2 | 2 Fe(OH)_3 | 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 KOH | 4 | -4 | -1/4 (Δ[KOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) K_2SO_4 | 2 | 2 | 1/2 (Δ[K2SO4])/(Δt) Fe(OH)_3 | 2 | 2 | 1/2 (Δ[Fe(OH)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 = -1/4 (Δ[KOH])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[FeSO4])/(Δt) = 1/2 (Δ[K2SO4])/(Δt) = 1/2 (Δ[Fe(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + H_2O_2 + FeSO_4 ⟶ K_2SO_4 + Fe(OH)_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: 4 KOH + H_2O_2 + 2 FeSO_4 ⟶ 2 K_2SO_4 + 2 Fe(OH)_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 KOH | 4 | -4 H_2O_2 | 1 | -1 FeSO_4 | 2 | -2 K_2SO_4 | 2 | 2 Fe(OH)_3 | 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 KOH | 4 | -4 | -1/4 (Δ[KOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) K_2SO_4 | 2 | 2 | 1/2 (Δ[K2SO4])/(Δt) Fe(OH)_3 | 2 | 2 | 1/2 (Δ[Fe(OH)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 = -1/4 (Δ[KOH])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[FeSO4])/(Δt) = 1/2 (Δ[K2SO4])/(Δt) = 1/2 (Δ[Fe(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | hydrogen peroxide | duretter | potassium sulfate | iron(III) hydroxide formula | KOH | H_2O_2 | FeSO_4 | K_2SO_4 | Fe(OH)_3 Hill formula | HKO | H_2O_2 | FeO_4S | K_2O_4S | FeH_3O_3 name | potassium hydroxide | hydrogen peroxide | duretter | potassium sulfate | iron(III) hydroxide IUPAC name | potassium hydroxide | hydrogen peroxide | iron(+2) cation sulfate | dipotassium sulfate | ferric trihydroxide
| potassium hydroxide | hydrogen peroxide | duretter | potassium sulfate | iron(III) hydroxide formula | KOH | H_2O_2 | FeSO_4 | K_2SO_4 | Fe(OH)_3 Hill formula | HKO | H_2O_2 | FeO_4S | K_2O_4S | FeH_3O_3 name | potassium hydroxide | hydrogen peroxide | duretter | potassium sulfate | iron(III) hydroxide IUPAC name | potassium hydroxide | hydrogen peroxide | iron(+2) cation sulfate | dipotassium sulfate | ferric trihydroxide

Substance properties

| potassium hydroxide | hydrogen peroxide | duretter | potassium sulfate | iron(III) hydroxide molar mass | 56.105 g/mol | 34.014 g/mol | 151.9 g/mol | 174.25 g/mol | 106.87 g/mol phase | solid (at STP) | liquid (at STP) | | | melting point | 406 °C | -0.43 °C | | | boiling point | 1327 °C | 150.2 °C | | | density | 2.044 g/cm^3 | 1.44 g/cm^3 | 2.841 g/cm^3 | | solubility in water | soluble | miscible | | soluble | surface tension | | 0.0804 N/m | | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.001249 Pa s (at 20 °C) | | |
| potassium hydroxide | hydrogen peroxide | duretter | potassium sulfate | iron(III) hydroxide molar mass | 56.105 g/mol | 34.014 g/mol | 151.9 g/mol | 174.25 g/mol | 106.87 g/mol phase | solid (at STP) | liquid (at STP) | | | melting point | 406 °C | -0.43 °C | | | boiling point | 1327 °C | 150.2 °C | | | density | 2.044 g/cm^3 | 1.44 g/cm^3 | 2.841 g/cm^3 | | solubility in water | soluble | miscible | | soluble | surface tension | | 0.0804 N/m | | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 0.001249 Pa s (at 20 °C) | | |

Units

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