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KOH + KMnO4 + KI = H2O + K2MnO4 + KIO4

Input interpretation

KOH (potassium hydroxide) + KMnO_4 (potassium permanganate) + KI (potassium iodide) ⟶ H_2O (water) + K_2MnO_4 (potassium manganate) + KIO_4 (potassium periodate)
KOH (potassium hydroxide) + KMnO_4 (potassium permanganate) + KI (potassium iodide) ⟶ H_2O (water) + K_2MnO_4 (potassium manganate) + KIO_4 (potassium periodate)

Balanced equation

Balance the chemical equation algebraically: KOH + KMnO_4 + KI ⟶ H_2O + K_2MnO_4 + KIO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KMnO_4 + c_3 KI ⟶ c_4 H_2O + c_5 K_2MnO_4 + c_6 KIO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Mn and I: H: | c_1 = 2 c_4 K: | c_1 + c_2 + c_3 = 2 c_5 + c_6 O: | c_1 + 4 c_2 = c_4 + 4 c_5 + 4 c_6 Mn: | c_2 = c_5 I: | c_3 = c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 8 c_3 = 1 c_4 = 4 c_5 = 8 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 KOH + 8 KMnO_4 + KI ⟶ 4 H_2O + 8 K_2MnO_4 + KIO_4
Balance the chemical equation algebraically: KOH + KMnO_4 + KI ⟶ H_2O + K_2MnO_4 + KIO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KMnO_4 + c_3 KI ⟶ c_4 H_2O + c_5 K_2MnO_4 + c_6 KIO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Mn and I: H: | c_1 = 2 c_4 K: | c_1 + c_2 + c_3 = 2 c_5 + c_6 O: | c_1 + 4 c_2 = c_4 + 4 c_5 + 4 c_6 Mn: | c_2 = c_5 I: | c_3 = c_6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 8 c_3 = 1 c_4 = 4 c_5 = 8 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 KOH + 8 KMnO_4 + KI ⟶ 4 H_2O + 8 K_2MnO_4 + KIO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

potassium hydroxide + potassium permanganate + potassium iodide ⟶ water + potassium manganate + potassium periodate
potassium hydroxide + potassium permanganate + potassium iodide ⟶ water + potassium manganate + potassium periodate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + KMnO_4 + KI ⟶ H_2O + K_2MnO_4 + KIO_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: 8 KOH + 8 KMnO_4 + KI ⟶ 4 H_2O + 8 K_2MnO_4 + KIO_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 KOH | 8 | -8 KMnO_4 | 8 | -8 KI | 1 | -1 H_2O | 4 | 4 K_2MnO_4 | 8 | 8 KIO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 8 | -8 | ([KOH])^(-8) KMnO_4 | 8 | -8 | ([KMnO4])^(-8) KI | 1 | -1 | ([KI])^(-1) H_2O | 4 | 4 | ([H2O])^4 K_2MnO_4 | 8 | 8 | ([K2MnO4])^8 KIO_4 | 1 | 1 | [KIO4] 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])^(-8) ([KMnO4])^(-8) ([KI])^(-1) ([H2O])^4 ([K2MnO4])^8 [KIO4] = (([H2O])^4 ([K2MnO4])^8 [KIO4])/(([KOH])^8 ([KMnO4])^8 [KI])
Construct the equilibrium constant, K, expression for: KOH + KMnO_4 + KI ⟶ H_2O + K_2MnO_4 + KIO_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: 8 KOH + 8 KMnO_4 + KI ⟶ 4 H_2O + 8 K_2MnO_4 + KIO_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 KOH | 8 | -8 KMnO_4 | 8 | -8 KI | 1 | -1 H_2O | 4 | 4 K_2MnO_4 | 8 | 8 KIO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 8 | -8 | ([KOH])^(-8) KMnO_4 | 8 | -8 | ([KMnO4])^(-8) KI | 1 | -1 | ([KI])^(-1) H_2O | 4 | 4 | ([H2O])^4 K_2MnO_4 | 8 | 8 | ([K2MnO4])^8 KIO_4 | 1 | 1 | [KIO4] 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])^(-8) ([KMnO4])^(-8) ([KI])^(-1) ([H2O])^4 ([K2MnO4])^8 [KIO4] = (([H2O])^4 ([K2MnO4])^8 [KIO4])/(([KOH])^8 ([KMnO4])^8 [KI])

Rate of reaction

Construct the rate of reaction expression for: KOH + KMnO_4 + KI ⟶ H_2O + K_2MnO_4 + KIO_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: 8 KOH + 8 KMnO_4 + KI ⟶ 4 H_2O + 8 K_2MnO_4 + KIO_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 KOH | 8 | -8 KMnO_4 | 8 | -8 KI | 1 | -1 H_2O | 4 | 4 K_2MnO_4 | 8 | 8 KIO_4 | 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 KOH | 8 | -8 | -1/8 (Δ[KOH])/(Δt) KMnO_4 | 8 | -8 | -1/8 (Δ[KMnO4])/(Δt) KI | 1 | -1 | -(Δ[KI])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2MnO_4 | 8 | 8 | 1/8 (Δ[K2MnO4])/(Δt) KIO_4 | 1 | 1 | (Δ[KIO4])/(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 = -1/8 (Δ[KOH])/(Δt) = -1/8 (Δ[KMnO4])/(Δt) = -(Δ[KI])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/8 (Δ[K2MnO4])/(Δt) = (Δ[KIO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + KMnO_4 + KI ⟶ H_2O + K_2MnO_4 + KIO_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: 8 KOH + 8 KMnO_4 + KI ⟶ 4 H_2O + 8 K_2MnO_4 + KIO_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 KOH | 8 | -8 KMnO_4 | 8 | -8 KI | 1 | -1 H_2O | 4 | 4 K_2MnO_4 | 8 | 8 KIO_4 | 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 KOH | 8 | -8 | -1/8 (Δ[KOH])/(Δt) KMnO_4 | 8 | -8 | -1/8 (Δ[KMnO4])/(Δt) KI | 1 | -1 | -(Δ[KI])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2MnO_4 | 8 | 8 | 1/8 (Δ[K2MnO4])/(Δt) KIO_4 | 1 | 1 | (Δ[KIO4])/(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 = -1/8 (Δ[KOH])/(Δt) = -1/8 (Δ[KMnO4])/(Δt) = -(Δ[KI])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/8 (Δ[K2MnO4])/(Δt) = (Δ[KIO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | potassium permanganate | potassium iodide | water | potassium manganate | potassium periodate formula | KOH | KMnO_4 | KI | H_2O | K_2MnO_4 | KIO_4 Hill formula | HKO | KMnO_4 | IK | H_2O | K_2MnO_4 | IKO_4 name | potassium hydroxide | potassium permanganate | potassium iodide | water | potassium manganate | potassium periodate IUPAC name | potassium hydroxide | potassium permanganate | potassium iodide | water | dipotassium dioxido-dioxomanganese | potassium periodate
| potassium hydroxide | potassium permanganate | potassium iodide | water | potassium manganate | potassium periodate formula | KOH | KMnO_4 | KI | H_2O | K_2MnO_4 | KIO_4 Hill formula | HKO | KMnO_4 | IK | H_2O | K_2MnO_4 | IKO_4 name | potassium hydroxide | potassium permanganate | potassium iodide | water | potassium manganate | potassium periodate IUPAC name | potassium hydroxide | potassium permanganate | potassium iodide | water | dipotassium dioxido-dioxomanganese | potassium periodate

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