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KOH + KMnO4 + CH3OH = H2O + K2MnO4 + KHCO3

Input interpretation

KOH potassium hydroxide + KMnO_4 potassium permanganate + CH_3OH methanol ⟶ H_2O water + K_2MnO_4 potassium manganate + KHCO_3 potassium bicarbonate
KOH potassium hydroxide + KMnO_4 potassium permanganate + CH_3OH methanol ⟶ H_2O water + K_2MnO_4 potassium manganate + KHCO_3 potassium bicarbonate

Balanced equation

Balance the chemical equation algebraically: KOH + KMnO_4 + CH_3OH ⟶ H_2O + K_2MnO_4 + KHCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KMnO_4 + c_3 CH_3OH ⟶ c_4 H_2O + c_5 K_2MnO_4 + c_6 KHCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Mn and C: H: | c_1 + 4 c_3 = 2 c_4 + c_6 K: | c_1 + c_2 = 2 c_5 + c_6 O: | c_1 + 4 c_2 + c_3 = c_4 + 4 c_5 + 3 c_6 Mn: | c_2 = c_5 C: | 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 = 7 c_2 = 6 c_3 = 1 c_4 = 5 c_5 = 6 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 KOH + 6 KMnO_4 + CH_3OH ⟶ 5 H_2O + 6 K_2MnO_4 + KHCO_3
Balance the chemical equation algebraically: KOH + KMnO_4 + CH_3OH ⟶ H_2O + K_2MnO_4 + KHCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KMnO_4 + c_3 CH_3OH ⟶ c_4 H_2O + c_5 K_2MnO_4 + c_6 KHCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Mn and C: H: | c_1 + 4 c_3 = 2 c_4 + c_6 K: | c_1 + c_2 = 2 c_5 + c_6 O: | c_1 + 4 c_2 + c_3 = c_4 + 4 c_5 + 3 c_6 Mn: | c_2 = c_5 C: | 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 = 7 c_2 = 6 c_3 = 1 c_4 = 5 c_5 = 6 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 KOH + 6 KMnO_4 + CH_3OH ⟶ 5 H_2O + 6 K_2MnO_4 + KHCO_3

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

potassium hydroxide + potassium permanganate + methanol ⟶ water + potassium manganate + potassium bicarbonate
potassium hydroxide + potassium permanganate + methanol ⟶ water + potassium manganate + potassium bicarbonate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + KMnO_4 + CH_3OH ⟶ H_2O + K_2MnO_4 + KHCO_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: 7 KOH + 6 KMnO_4 + CH_3OH ⟶ 5 H_2O + 6 K_2MnO_4 + KHCO_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 | 7 | -7 KMnO_4 | 6 | -6 CH_3OH | 1 | -1 H_2O | 5 | 5 K_2MnO_4 | 6 | 6 KHCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 7 | -7 | ([KOH])^(-7) KMnO_4 | 6 | -6 | ([KMnO4])^(-6) CH_3OH | 1 | -1 | ([CH3OH])^(-1) H_2O | 5 | 5 | ([H2O])^5 K_2MnO_4 | 6 | 6 | ([K2MnO4])^6 KHCO_3 | 1 | 1 | [KHCO3] 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])^(-7) ([KMnO4])^(-6) ([CH3OH])^(-1) ([H2O])^5 ([K2MnO4])^6 [KHCO3] = (([H2O])^5 ([K2MnO4])^6 [KHCO3])/(([KOH])^7 ([KMnO4])^6 [CH3OH])
Construct the equilibrium constant, K, expression for: KOH + KMnO_4 + CH_3OH ⟶ H_2O + K_2MnO_4 + KHCO_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: 7 KOH + 6 KMnO_4 + CH_3OH ⟶ 5 H_2O + 6 K_2MnO_4 + KHCO_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 | 7 | -7 KMnO_4 | 6 | -6 CH_3OH | 1 | -1 H_2O | 5 | 5 K_2MnO_4 | 6 | 6 KHCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 7 | -7 | ([KOH])^(-7) KMnO_4 | 6 | -6 | ([KMnO4])^(-6) CH_3OH | 1 | -1 | ([CH3OH])^(-1) H_2O | 5 | 5 | ([H2O])^5 K_2MnO_4 | 6 | 6 | ([K2MnO4])^6 KHCO_3 | 1 | 1 | [KHCO3] 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])^(-7) ([KMnO4])^(-6) ([CH3OH])^(-1) ([H2O])^5 ([K2MnO4])^6 [KHCO3] = (([H2O])^5 ([K2MnO4])^6 [KHCO3])/(([KOH])^7 ([KMnO4])^6 [CH3OH])

Rate of reaction

Construct the rate of reaction expression for: KOH + KMnO_4 + CH_3OH ⟶ H_2O + K_2MnO_4 + KHCO_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: 7 KOH + 6 KMnO_4 + CH_3OH ⟶ 5 H_2O + 6 K_2MnO_4 + KHCO_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 | 7 | -7 KMnO_4 | 6 | -6 CH_3OH | 1 | -1 H_2O | 5 | 5 K_2MnO_4 | 6 | 6 KHCO_3 | 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 | 7 | -7 | -1/7 (Δ[KOH])/(Δt) KMnO_4 | 6 | -6 | -1/6 (Δ[KMnO4])/(Δt) CH_3OH | 1 | -1 | -(Δ[CH3OH])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K_2MnO_4 | 6 | 6 | 1/6 (Δ[K2MnO4])/(Δt) KHCO_3 | 1 | 1 | (Δ[KHCO3])/(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 = -1/7 (Δ[KOH])/(Δt) = -1/6 (Δ[KMnO4])/(Δt) = -(Δ[CH3OH])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/6 (Δ[K2MnO4])/(Δt) = (Δ[KHCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + KMnO_4 + CH_3OH ⟶ H_2O + K_2MnO_4 + KHCO_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: 7 KOH + 6 KMnO_4 + CH_3OH ⟶ 5 H_2O + 6 K_2MnO_4 + KHCO_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 | 7 | -7 KMnO_4 | 6 | -6 CH_3OH | 1 | -1 H_2O | 5 | 5 K_2MnO_4 | 6 | 6 KHCO_3 | 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 | 7 | -7 | -1/7 (Δ[KOH])/(Δt) KMnO_4 | 6 | -6 | -1/6 (Δ[KMnO4])/(Δt) CH_3OH | 1 | -1 | -(Δ[CH3OH])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K_2MnO_4 | 6 | 6 | 1/6 (Δ[K2MnO4])/(Δt) KHCO_3 | 1 | 1 | (Δ[KHCO3])/(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 = -1/7 (Δ[KOH])/(Δt) = -1/6 (Δ[KMnO4])/(Δt) = -(Δ[CH3OH])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/6 (Δ[K2MnO4])/(Δt) = (Δ[KHCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | potassium permanganate | methanol | water | potassium manganate | potassium bicarbonate formula | KOH | KMnO_4 | CH_3OH | H_2O | K_2MnO_4 | KHCO_3 Hill formula | HKO | KMnO_4 | CH_4O | H_2O | K_2MnO_4 | CHKO_3 name | potassium hydroxide | potassium permanganate | methanol | water | potassium manganate | potassium bicarbonate IUPAC name | potassium hydroxide | potassium permanganate | methanol | water | dipotassium dioxido-dioxomanganese | potassium hydrogen carbonate
| potassium hydroxide | potassium permanganate | methanol | water | potassium manganate | potassium bicarbonate formula | KOH | KMnO_4 | CH_3OH | H_2O | K_2MnO_4 | KHCO_3 Hill formula | HKO | KMnO_4 | CH_4O | H_2O | K_2MnO_4 | CHKO_3 name | potassium hydroxide | potassium permanganate | methanol | water | potassium manganate | potassium bicarbonate IUPAC name | potassium hydroxide | potassium permanganate | methanol | water | dipotassium dioxido-dioxomanganese | potassium hydrogen carbonate

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