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KMnO4 + FeCl2 + H2(SO4) = H2O + Cl2 + K2SO4 + MnSO4 + Fe2(SO4)3

Input interpretation

KMnO_4 potassium permanganate + FeCl_2 iron(II) chloride + H_2SO_4 sulfuric acid ⟶ H_2O water + Cl_2 chlorine + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate
KMnO_4 potassium permanganate + FeCl_2 iron(II) chloride + H_2SO_4 sulfuric acid ⟶ H_2O water + Cl_2 chlorine + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate

Balanced equation

Balance the chemical equation algebraically: KMnO_4 + FeCl_2 + H_2SO_4 ⟶ H_2O + Cl_2 + K_2SO_4 + MnSO_4 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 FeCl_2 + c_3 H_2SO_4 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 K_2SO_4 + c_7 MnSO_4 + c_8 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 K, Mn, O, Cl, Fe, H and S: K: | c_1 = 2 c_6 Mn: | c_1 = c_7 O: | 4 c_1 + 4 c_3 = c_4 + 4 c_6 + 4 c_7 + 12 c_8 Cl: | 2 c_2 = 2 c_5 Fe: | c_2 = 2 c_8 H: | 2 c_3 = 2 c_4 S: | c_3 = c_6 + c_7 + 3 c_8 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 10/3 c_3 = 8 c_4 = 8 c_5 = 10/3 c_6 = 1 c_7 = 2 c_8 = 5/3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 6 c_2 = 10 c_3 = 24 c_4 = 24 c_5 = 10 c_6 = 3 c_7 = 6 c_8 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KMnO_4 + 10 FeCl_2 + 24 H_2SO_4 ⟶ 24 H_2O + 10 Cl_2 + 3 K_2SO_4 + 6 MnSO_4 + 5 Fe_2(SO_4)_3·xH_2O
Balance the chemical equation algebraically: KMnO_4 + FeCl_2 + H_2SO_4 ⟶ H_2O + Cl_2 + K_2SO_4 + MnSO_4 + Fe_2(SO_4)_3·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 FeCl_2 + c_3 H_2SO_4 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 K_2SO_4 + c_7 MnSO_4 + c_8 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 K, Mn, O, Cl, Fe, H and S: K: | c_1 = 2 c_6 Mn: | c_1 = c_7 O: | 4 c_1 + 4 c_3 = c_4 + 4 c_6 + 4 c_7 + 12 c_8 Cl: | 2 c_2 = 2 c_5 Fe: | c_2 = 2 c_8 H: | 2 c_3 = 2 c_4 S: | c_3 = c_6 + c_7 + 3 c_8 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 10/3 c_3 = 8 c_4 = 8 c_5 = 10/3 c_6 = 1 c_7 = 2 c_8 = 5/3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 6 c_2 = 10 c_3 = 24 c_4 = 24 c_5 = 10 c_6 = 3 c_7 = 6 c_8 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KMnO_4 + 10 FeCl_2 + 24 H_2SO_4 ⟶ 24 H_2O + 10 Cl_2 + 3 K_2SO_4 + 6 MnSO_4 + 5 Fe_2(SO_4)_3·xH_2O

Structures

+ + ⟶ + + + +
+ + ⟶ + + + +

Names

potassium permanganate + iron(II) chloride + sulfuric acid ⟶ water + chlorine + potassium sulfate + manganese(II) sulfate + iron(III) sulfate hydrate
potassium permanganate + iron(II) chloride + sulfuric acid ⟶ water + chlorine + potassium sulfate + manganese(II) sulfate + iron(III) sulfate hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KMnO_4 + FeCl_2 + H_2SO_4 ⟶ H_2O + Cl_2 + K_2SO_4 + MnSO_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: 6 KMnO_4 + 10 FeCl_2 + 24 H_2SO_4 ⟶ 24 H_2O + 10 Cl_2 + 3 K_2SO_4 + 6 MnSO_4 + 5 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 KMnO_4 | 6 | -6 FeCl_2 | 10 | -10 H_2SO_4 | 24 | -24 H_2O | 24 | 24 Cl_2 | 10 | 10 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 Fe_2(SO_4)_3·xH_2O | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 6 | -6 | ([KMnO4])^(-6) FeCl_2 | 10 | -10 | ([FeCl2])^(-10) H_2SO_4 | 24 | -24 | ([H2SO4])^(-24) H_2O | 24 | 24 | ([H2O])^24 Cl_2 | 10 | 10 | ([Cl2])^10 K_2SO_4 | 3 | 3 | ([K2SO4])^3 MnSO_4 | 6 | 6 | ([MnSO4])^6 Fe_2(SO_4)_3·xH_2O | 5 | 5 | ([Fe2(SO4)3·xH2O])^5 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 = ([KMnO4])^(-6) ([FeCl2])^(-10) ([H2SO4])^(-24) ([H2O])^24 ([Cl2])^10 ([K2SO4])^3 ([MnSO4])^6 ([Fe2(SO4)3·xH2O])^5 = (([H2O])^24 ([Cl2])^10 ([K2SO4])^3 ([MnSO4])^6 ([Fe2(SO4)3·xH2O])^5)/(([KMnO4])^6 ([FeCl2])^10 ([H2SO4])^24)
Construct the equilibrium constant, K, expression for: KMnO_4 + FeCl_2 + H_2SO_4 ⟶ H_2O + Cl_2 + K_2SO_4 + MnSO_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: 6 KMnO_4 + 10 FeCl_2 + 24 H_2SO_4 ⟶ 24 H_2O + 10 Cl_2 + 3 K_2SO_4 + 6 MnSO_4 + 5 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 KMnO_4 | 6 | -6 FeCl_2 | 10 | -10 H_2SO_4 | 24 | -24 H_2O | 24 | 24 Cl_2 | 10 | 10 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 Fe_2(SO_4)_3·xH_2O | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 6 | -6 | ([KMnO4])^(-6) FeCl_2 | 10 | -10 | ([FeCl2])^(-10) H_2SO_4 | 24 | -24 | ([H2SO4])^(-24) H_2O | 24 | 24 | ([H2O])^24 Cl_2 | 10 | 10 | ([Cl2])^10 K_2SO_4 | 3 | 3 | ([K2SO4])^3 MnSO_4 | 6 | 6 | ([MnSO4])^6 Fe_2(SO_4)_3·xH_2O | 5 | 5 | ([Fe2(SO4)3·xH2O])^5 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 = ([KMnO4])^(-6) ([FeCl2])^(-10) ([H2SO4])^(-24) ([H2O])^24 ([Cl2])^10 ([K2SO4])^3 ([MnSO4])^6 ([Fe2(SO4)3·xH2O])^5 = (([H2O])^24 ([Cl2])^10 ([K2SO4])^3 ([MnSO4])^6 ([Fe2(SO4)3·xH2O])^5)/(([KMnO4])^6 ([FeCl2])^10 ([H2SO4])^24)

Rate of reaction

Construct the rate of reaction expression for: KMnO_4 + FeCl_2 + H_2SO_4 ⟶ H_2O + Cl_2 + K_2SO_4 + MnSO_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: 6 KMnO_4 + 10 FeCl_2 + 24 H_2SO_4 ⟶ 24 H_2O + 10 Cl_2 + 3 K_2SO_4 + 6 MnSO_4 + 5 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 KMnO_4 | 6 | -6 FeCl_2 | 10 | -10 H_2SO_4 | 24 | -24 H_2O | 24 | 24 Cl_2 | 10 | 10 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 Fe_2(SO_4)_3·xH_2O | 5 | 5 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 KMnO_4 | 6 | -6 | -1/6 (Δ[KMnO4])/(Δt) FeCl_2 | 10 | -10 | -1/10 (Δ[FeCl2])/(Δt) H_2SO_4 | 24 | -24 | -1/24 (Δ[H2SO4])/(Δt) H_2O | 24 | 24 | 1/24 (Δ[H2O])/(Δt) Cl_2 | 10 | 10 | 1/10 (Δ[Cl2])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) MnSO_4 | 6 | 6 | 1/6 (Δ[MnSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 5 | 5 | 1/5 (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 = -1/6 (Δ[KMnO4])/(Δt) = -1/10 (Δ[FeCl2])/(Δt) = -1/24 (Δ[H2SO4])/(Δt) = 1/24 (Δ[H2O])/(Δt) = 1/10 (Δ[Cl2])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/6 (Δ[MnSO4])/(Δt) = 1/5 (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KMnO_4 + FeCl_2 + H_2SO_4 ⟶ H_2O + Cl_2 + K_2SO_4 + MnSO_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: 6 KMnO_4 + 10 FeCl_2 + 24 H_2SO_4 ⟶ 24 H_2O + 10 Cl_2 + 3 K_2SO_4 + 6 MnSO_4 + 5 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 KMnO_4 | 6 | -6 FeCl_2 | 10 | -10 H_2SO_4 | 24 | -24 H_2O | 24 | 24 Cl_2 | 10 | 10 K_2SO_4 | 3 | 3 MnSO_4 | 6 | 6 Fe_2(SO_4)_3·xH_2O | 5 | 5 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 KMnO_4 | 6 | -6 | -1/6 (Δ[KMnO4])/(Δt) FeCl_2 | 10 | -10 | -1/10 (Δ[FeCl2])/(Δt) H_2SO_4 | 24 | -24 | -1/24 (Δ[H2SO4])/(Δt) H_2O | 24 | 24 | 1/24 (Δ[H2O])/(Δt) Cl_2 | 10 | 10 | 1/10 (Δ[Cl2])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) MnSO_4 | 6 | 6 | 1/6 (Δ[MnSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 5 | 5 | 1/5 (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 = -1/6 (Δ[KMnO4])/(Δt) = -1/10 (Δ[FeCl2])/(Δt) = -1/24 (Δ[H2SO4])/(Δt) = 1/24 (Δ[H2O])/(Δt) = 1/10 (Δ[Cl2])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/6 (Δ[MnSO4])/(Δt) = 1/5 (Δ[Fe2(SO4)3·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium permanganate | iron(II) chloride | sulfuric acid | water | chlorine | potassium sulfate | manganese(II) sulfate | iron(III) sulfate hydrate formula | KMnO_4 | FeCl_2 | H_2SO_4 | H_2O | Cl_2 | K_2SO_4 | MnSO_4 | Fe_2(SO_4)_3·xH_2O Hill formula | KMnO_4 | Cl_2Fe | H_2O_4S | H_2O | Cl_2 | K_2O_4S | MnSO_4 | Fe_2O_12S_3 name | potassium permanganate | iron(II) chloride | sulfuric acid | water | chlorine | potassium sulfate | manganese(II) sulfate | iron(III) sulfate hydrate IUPAC name | potassium permanganate | dichloroiron | sulfuric acid | water | molecular chlorine | dipotassium sulfate | manganese(+2) cation sulfate | diferric trisulfate
| potassium permanganate | iron(II) chloride | sulfuric acid | water | chlorine | potassium sulfate | manganese(II) sulfate | iron(III) sulfate hydrate formula | KMnO_4 | FeCl_2 | H_2SO_4 | H_2O | Cl_2 | K_2SO_4 | MnSO_4 | Fe_2(SO_4)_3·xH_2O Hill formula | KMnO_4 | Cl_2Fe | H_2O_4S | H_2O | Cl_2 | K_2O_4S | MnSO_4 | Fe_2O_12S_3 name | potassium permanganate | iron(II) chloride | sulfuric acid | water | chlorine | potassium sulfate | manganese(II) sulfate | iron(III) sulfate hydrate IUPAC name | potassium permanganate | dichloroiron | sulfuric acid | water | molecular chlorine | dipotassium sulfate | manganese(+2) cation sulfate | diferric trisulfate

Substance properties

| potassium permanganate | iron(II) chloride | sulfuric acid | water | chlorine | potassium sulfate | manganese(II) sulfate | iron(III) sulfate hydrate molar mass | 158.03 g/mol | 126.7 g/mol | 98.07 g/mol | 18.015 g/mol | 70.9 g/mol | 174.25 g/mol | 150.99 g/mol | 399.9 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | | solid (at STP) | melting point | 240 °C | 677 °C | 10.371 °C | 0 °C | -101 °C | | 710 °C | boiling point | | | 279.6 °C | 99.9839 °C | -34 °C | | | density | 1 g/cm^3 | 3.16 g/cm^3 | 1.8305 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | | 3.25 g/cm^3 | solubility in water | | | very soluble | | | soluble | 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 | odorless | | | |
| potassium permanganate | iron(II) chloride | sulfuric acid | water | chlorine | potassium sulfate | manganese(II) sulfate | iron(III) sulfate hydrate molar mass | 158.03 g/mol | 126.7 g/mol | 98.07 g/mol | 18.015 g/mol | 70.9 g/mol | 174.25 g/mol | 150.99 g/mol | 399.9 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | | solid (at STP) | melting point | 240 °C | 677 °C | 10.371 °C | 0 °C | -101 °C | | 710 °C | boiling point | | | 279.6 °C | 99.9839 °C | -34 °C | | | density | 1 g/cm^3 | 3.16 g/cm^3 | 1.8305 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | | 3.25 g/cm^3 | solubility in water | | | very soluble | | | soluble | 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 | odorless | | | |

Units

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