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KMnO4 + Na2SO3 + H2SO3 = H2O + K2SO4 + Na2SO4 + MnSO4

Input interpretation

KMnO_4 potassium permanganate + Na_2SO_3 sodium sulfite + H_2SO_3 sulfurous acid ⟶ H_2O water + K_2SO_4 potassium sulfate + Na_2SO_4 sodium sulfate + MnSO_4 manganese(II) sulfate
KMnO_4 potassium permanganate + Na_2SO_3 sodium sulfite + H_2SO_3 sulfurous acid ⟶ H_2O water + K_2SO_4 potassium sulfate + Na_2SO_4 sodium sulfate + MnSO_4 manganese(II) sulfate

Balanced equation

Balance the chemical equation algebraically: KMnO_4 + Na_2SO_3 + H_2SO_3 ⟶ H_2O + K_2SO_4 + Na_2SO_4 + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 Na_2SO_3 + c_3 H_2SO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 Na_2SO_4 + c_7 MnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, Na, S and H: K: | c_1 = 2 c_5 Mn: | c_1 = c_7 O: | 4 c_1 + 3 c_2 + 3 c_3 = c_4 + 4 c_5 + 4 c_6 + 4 c_7 Na: | 2 c_2 = 2 c_6 S: | c_2 + c_3 = c_5 + c_6 + c_7 H: | 2 c_3 = 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 3 c_4 = 3 c_5 = 1 c_6 = 2 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KMnO_4 + 2 Na_2SO_3 + 3 H_2SO_3 ⟶ 3 H_2O + K_2SO_4 + 2 Na_2SO_4 + 2 MnSO_4
Balance the chemical equation algebraically: KMnO_4 + Na_2SO_3 + H_2SO_3 ⟶ H_2O + K_2SO_4 + Na_2SO_4 + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 Na_2SO_3 + c_3 H_2SO_3 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 Na_2SO_4 + c_7 MnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, Na, S and H: K: | c_1 = 2 c_5 Mn: | c_1 = c_7 O: | 4 c_1 + 3 c_2 + 3 c_3 = c_4 + 4 c_5 + 4 c_6 + 4 c_7 Na: | 2 c_2 = 2 c_6 S: | c_2 + c_3 = c_5 + c_6 + c_7 H: | 2 c_3 = 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 3 c_4 = 3 c_5 = 1 c_6 = 2 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KMnO_4 + 2 Na_2SO_3 + 3 H_2SO_3 ⟶ 3 H_2O + K_2SO_4 + 2 Na_2SO_4 + 2 MnSO_4

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

potassium permanganate + sodium sulfite + sulfurous acid ⟶ water + potassium sulfate + sodium sulfate + manganese(II) sulfate
potassium permanganate + sodium sulfite + sulfurous acid ⟶ water + potassium sulfate + sodium sulfate + manganese(II) sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KMnO_4 + Na_2SO_3 + H_2SO_3 ⟶ H_2O + K_2SO_4 + Na_2SO_4 + MnSO_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: 2 KMnO_4 + 2 Na_2SO_3 + 3 H_2SO_3 ⟶ 3 H_2O + K_2SO_4 + 2 Na_2SO_4 + 2 MnSO_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 KMnO_4 | 2 | -2 Na_2SO_3 | 2 | -2 H_2SO_3 | 3 | -3 H_2O | 3 | 3 K_2SO_4 | 1 | 1 Na_2SO_4 | 2 | 2 MnSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 2 | -2 | ([KMnO4])^(-2) Na_2SO_3 | 2 | -2 | ([Na2SO3])^(-2) H_2SO_3 | 3 | -3 | ([H2SO3])^(-3) H_2O | 3 | 3 | ([H2O])^3 K_2SO_4 | 1 | 1 | [K2SO4] Na_2SO_4 | 2 | 2 | ([Na2SO4])^2 MnSO_4 | 2 | 2 | ([MnSO4])^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 = ([KMnO4])^(-2) ([Na2SO3])^(-2) ([H2SO3])^(-3) ([H2O])^3 [K2SO4] ([Na2SO4])^2 ([MnSO4])^2 = (([H2O])^3 [K2SO4] ([Na2SO4])^2 ([MnSO4])^2)/(([KMnO4])^2 ([Na2SO3])^2 ([H2SO3])^3)
Construct the equilibrium constant, K, expression for: KMnO_4 + Na_2SO_3 + H_2SO_3 ⟶ H_2O + K_2SO_4 + Na_2SO_4 + MnSO_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: 2 KMnO_4 + 2 Na_2SO_3 + 3 H_2SO_3 ⟶ 3 H_2O + K_2SO_4 + 2 Na_2SO_4 + 2 MnSO_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 KMnO_4 | 2 | -2 Na_2SO_3 | 2 | -2 H_2SO_3 | 3 | -3 H_2O | 3 | 3 K_2SO_4 | 1 | 1 Na_2SO_4 | 2 | 2 MnSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 2 | -2 | ([KMnO4])^(-2) Na_2SO_3 | 2 | -2 | ([Na2SO3])^(-2) H_2SO_3 | 3 | -3 | ([H2SO3])^(-3) H_2O | 3 | 3 | ([H2O])^3 K_2SO_4 | 1 | 1 | [K2SO4] Na_2SO_4 | 2 | 2 | ([Na2SO4])^2 MnSO_4 | 2 | 2 | ([MnSO4])^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 = ([KMnO4])^(-2) ([Na2SO3])^(-2) ([H2SO3])^(-3) ([H2O])^3 [K2SO4] ([Na2SO4])^2 ([MnSO4])^2 = (([H2O])^3 [K2SO4] ([Na2SO4])^2 ([MnSO4])^2)/(([KMnO4])^2 ([Na2SO3])^2 ([H2SO3])^3)

Rate of reaction

Construct the rate of reaction expression for: KMnO_4 + Na_2SO_3 + H_2SO_3 ⟶ H_2O + K_2SO_4 + Na_2SO_4 + MnSO_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: 2 KMnO_4 + 2 Na_2SO_3 + 3 H_2SO_3 ⟶ 3 H_2O + K_2SO_4 + 2 Na_2SO_4 + 2 MnSO_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 KMnO_4 | 2 | -2 Na_2SO_3 | 2 | -2 H_2SO_3 | 3 | -3 H_2O | 3 | 3 K_2SO_4 | 1 | 1 Na_2SO_4 | 2 | 2 MnSO_4 | 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 KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) Na_2SO_3 | 2 | -2 | -1/2 (Δ[Na2SO3])/(Δt) H_2SO_3 | 3 | -3 | -1/3 (Δ[H2SO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Na_2SO_4 | 2 | 2 | 1/2 (Δ[Na2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(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 = -1/2 (Δ[KMnO4])/(Δt) = -1/2 (Δ[Na2SO3])/(Δt) = -1/3 (Δ[H2SO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[Na2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KMnO_4 + Na_2SO_3 + H_2SO_3 ⟶ H_2O + K_2SO_4 + Na_2SO_4 + MnSO_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: 2 KMnO_4 + 2 Na_2SO_3 + 3 H_2SO_3 ⟶ 3 H_2O + K_2SO_4 + 2 Na_2SO_4 + 2 MnSO_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 KMnO_4 | 2 | -2 Na_2SO_3 | 2 | -2 H_2SO_3 | 3 | -3 H_2O | 3 | 3 K_2SO_4 | 1 | 1 Na_2SO_4 | 2 | 2 MnSO_4 | 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 KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) Na_2SO_3 | 2 | -2 | -1/2 (Δ[Na2SO3])/(Δt) H_2SO_3 | 3 | -3 | -1/3 (Δ[H2SO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Na_2SO_4 | 2 | 2 | 1/2 (Δ[Na2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(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 = -1/2 (Δ[KMnO4])/(Δt) = -1/2 (Δ[Na2SO3])/(Δt) = -1/3 (Δ[H2SO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[Na2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium permanganate | sodium sulfite | sulfurous acid | water | potassium sulfate | sodium sulfate | manganese(II) sulfate formula | KMnO_4 | Na_2SO_3 | H_2SO_3 | H_2O | K_2SO_4 | Na_2SO_4 | MnSO_4 Hill formula | KMnO_4 | Na_2O_3S | H_2O_3S | H_2O | K_2O_4S | Na_2O_4S | MnSO_4 name | potassium permanganate | sodium sulfite | sulfurous acid | water | potassium sulfate | sodium sulfate | manganese(II) sulfate IUPAC name | potassium permanganate | disodium sulfite | sulfurous acid | water | dipotassium sulfate | disodium sulfate | manganese(+2) cation sulfate
| potassium permanganate | sodium sulfite | sulfurous acid | water | potassium sulfate | sodium sulfate | manganese(II) sulfate formula | KMnO_4 | Na_2SO_3 | H_2SO_3 | H_2O | K_2SO_4 | Na_2SO_4 | MnSO_4 Hill formula | KMnO_4 | Na_2O_3S | H_2O_3S | H_2O | K_2O_4S | Na_2O_4S | MnSO_4 name | potassium permanganate | sodium sulfite | sulfurous acid | water | potassium sulfate | sodium sulfate | manganese(II) sulfate IUPAC name | potassium permanganate | disodium sulfite | sulfurous acid | water | dipotassium sulfate | disodium sulfate | manganese(+2) cation sulfate

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