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KMnO4 + H2S = H2O + K2SO4 + KOH + MnO2

Input interpretation

KMnO_4 potassium permanganate + H_2S hydrogen sulfide ⟶ H_2O water + K_2SO_4 potassium sulfate + KOH potassium hydroxide + MnO_2 manganese dioxide
KMnO_4 potassium permanganate + H_2S hydrogen sulfide ⟶ H_2O water + K_2SO_4 potassium sulfate + KOH potassium hydroxide + MnO_2 manganese dioxide

Balanced equation

Balance the chemical equation algebraically: KMnO_4 + H_2S ⟶ H_2O + K_2SO_4 + KOH + MnO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 H_2S ⟶ c_3 H_2O + c_4 K_2SO_4 + c_5 KOH + c_6 MnO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, H and S: K: | c_1 = 2 c_4 + c_5 Mn: | c_1 = c_6 O: | 4 c_1 = c_3 + 4 c_4 + c_5 + 2 c_6 H: | 2 c_2 = 2 c_3 + c_5 S: | c_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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 3/2 c_3 = 1 c_4 = 3/2 c_5 = 1 c_6 = 4 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 3 c_3 = 2 c_4 = 3 c_5 = 2 c_6 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 KMnO_4 + 3 H_2S ⟶ 2 H_2O + 3 K_2SO_4 + 2 KOH + 8 MnO_2
Balance the chemical equation algebraically: KMnO_4 + H_2S ⟶ H_2O + K_2SO_4 + KOH + MnO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 H_2S ⟶ c_3 H_2O + c_4 K_2SO_4 + c_5 KOH + c_6 MnO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, H and S: K: | c_1 = 2 c_4 + c_5 Mn: | c_1 = c_6 O: | 4 c_1 = c_3 + 4 c_4 + c_5 + 2 c_6 H: | 2 c_2 = 2 c_3 + c_5 S: | c_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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 3/2 c_3 = 1 c_4 = 3/2 c_5 = 1 c_6 = 4 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 3 c_3 = 2 c_4 = 3 c_5 = 2 c_6 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 KMnO_4 + 3 H_2S ⟶ 2 H_2O + 3 K_2SO_4 + 2 KOH + 8 MnO_2

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

potassium permanganate + hydrogen sulfide ⟶ water + potassium sulfate + potassium hydroxide + manganese dioxide
potassium permanganate + hydrogen sulfide ⟶ water + potassium sulfate + potassium hydroxide + manganese dioxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KMnO_4 + H_2S ⟶ H_2O + K_2SO_4 + KOH + MnO_2 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 KMnO_4 + 3 H_2S ⟶ 2 H_2O + 3 K_2SO_4 + 2 KOH + 8 MnO_2 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 | 8 | -8 H_2S | 3 | -3 H_2O | 2 | 2 K_2SO_4 | 3 | 3 KOH | 2 | 2 MnO_2 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 8 | -8 | ([KMnO4])^(-8) H_2S | 3 | -3 | ([H2S])^(-3) H_2O | 2 | 2 | ([H2O])^2 K_2SO_4 | 3 | 3 | ([K2SO4])^3 KOH | 2 | 2 | ([KOH])^2 MnO_2 | 8 | 8 | ([MnO2])^8 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])^(-8) ([H2S])^(-3) ([H2O])^2 ([K2SO4])^3 ([KOH])^2 ([MnO2])^8 = (([H2O])^2 ([K2SO4])^3 ([KOH])^2 ([MnO2])^8)/(([KMnO4])^8 ([H2S])^3)
Construct the equilibrium constant, K, expression for: KMnO_4 + H_2S ⟶ H_2O + K_2SO_4 + KOH + MnO_2 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 KMnO_4 + 3 H_2S ⟶ 2 H_2O + 3 K_2SO_4 + 2 KOH + 8 MnO_2 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 | 8 | -8 H_2S | 3 | -3 H_2O | 2 | 2 K_2SO_4 | 3 | 3 KOH | 2 | 2 MnO_2 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 8 | -8 | ([KMnO4])^(-8) H_2S | 3 | -3 | ([H2S])^(-3) H_2O | 2 | 2 | ([H2O])^2 K_2SO_4 | 3 | 3 | ([K2SO4])^3 KOH | 2 | 2 | ([KOH])^2 MnO_2 | 8 | 8 | ([MnO2])^8 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])^(-8) ([H2S])^(-3) ([H2O])^2 ([K2SO4])^3 ([KOH])^2 ([MnO2])^8 = (([H2O])^2 ([K2SO4])^3 ([KOH])^2 ([MnO2])^8)/(([KMnO4])^8 ([H2S])^3)

Rate of reaction

Construct the rate of reaction expression for: KMnO_4 + H_2S ⟶ H_2O + K_2SO_4 + KOH + MnO_2 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 KMnO_4 + 3 H_2S ⟶ 2 H_2O + 3 K_2SO_4 + 2 KOH + 8 MnO_2 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 | 8 | -8 H_2S | 3 | -3 H_2O | 2 | 2 K_2SO_4 | 3 | 3 KOH | 2 | 2 MnO_2 | 8 | 8 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 | 8 | -8 | -1/8 (Δ[KMnO4])/(Δt) H_2S | 3 | -3 | -1/3 (Δ[H2S])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) MnO_2 | 8 | 8 | 1/8 (Δ[MnO2])/(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[KMnO4])/(Δt) = -1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/2 (Δ[KOH])/(Δt) = 1/8 (Δ[MnO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KMnO_4 + H_2S ⟶ H_2O + K_2SO_4 + KOH + MnO_2 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 KMnO_4 + 3 H_2S ⟶ 2 H_2O + 3 K_2SO_4 + 2 KOH + 8 MnO_2 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 | 8 | -8 H_2S | 3 | -3 H_2O | 2 | 2 K_2SO_4 | 3 | 3 KOH | 2 | 2 MnO_2 | 8 | 8 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 | 8 | -8 | -1/8 (Δ[KMnO4])/(Δt) H_2S | 3 | -3 | -1/3 (Δ[H2S])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) MnO_2 | 8 | 8 | 1/8 (Δ[MnO2])/(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[KMnO4])/(Δt) = -1/3 (Δ[H2S])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/2 (Δ[KOH])/(Δt) = 1/8 (Δ[MnO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium permanganate | hydrogen sulfide | water | potassium sulfate | potassium hydroxide | manganese dioxide formula | KMnO_4 | H_2S | H_2O | K_2SO_4 | KOH | MnO_2 Hill formula | KMnO_4 | H_2S | H_2O | K_2O_4S | HKO | MnO_2 name | potassium permanganate | hydrogen sulfide | water | potassium sulfate | potassium hydroxide | manganese dioxide IUPAC name | potassium permanganate | hydrogen sulfide | water | dipotassium sulfate | potassium hydroxide | dioxomanganese
| potassium permanganate | hydrogen sulfide | water | potassium sulfate | potassium hydroxide | manganese dioxide formula | KMnO_4 | H_2S | H_2O | K_2SO_4 | KOH | MnO_2 Hill formula | KMnO_4 | H_2S | H_2O | K_2O_4S | HKO | MnO_2 name | potassium permanganate | hydrogen sulfide | water | potassium sulfate | potassium hydroxide | manganese dioxide IUPAC name | potassium permanganate | hydrogen sulfide | water | dipotassium sulfate | potassium hydroxide | dioxomanganese

Substance properties

| potassium permanganate | hydrogen sulfide | water | potassium sulfate | potassium hydroxide | manganese dioxide molar mass | 158.03 g/mol | 34.08 g/mol | 18.015 g/mol | 174.25 g/mol | 56.105 g/mol | 86.936 g/mol phase | solid (at STP) | gas (at STP) | liquid (at STP) | | solid (at STP) | solid (at STP) melting point | 240 °C | -85 °C | 0 °C | | 406 °C | 535 °C boiling point | | -60 °C | 99.9839 °C | | 1327 °C | density | 1 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 1 g/cm^3 | | 2.044 g/cm^3 | 5.03 g/cm^3 solubility in water | | | | soluble | soluble | insoluble surface tension | | | 0.0728 N/m | | | dynamic viscosity | | 1.239×10^-5 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | | 0.001 Pa s (at 550 °C) | odor | odorless | | odorless | | |
| potassium permanganate | hydrogen sulfide | water | potassium sulfate | potassium hydroxide | manganese dioxide molar mass | 158.03 g/mol | 34.08 g/mol | 18.015 g/mol | 174.25 g/mol | 56.105 g/mol | 86.936 g/mol phase | solid (at STP) | gas (at STP) | liquid (at STP) | | solid (at STP) | solid (at STP) melting point | 240 °C | -85 °C | 0 °C | | 406 °C | 535 °C boiling point | | -60 °C | 99.9839 °C | | 1327 °C | density | 1 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 1 g/cm^3 | | 2.044 g/cm^3 | 5.03 g/cm^3 solubility in water | | | | soluble | soluble | insoluble surface tension | | | 0.0728 N/m | | | dynamic viscosity | | 1.239×10^-5 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | | 0.001 Pa s (at 550 °C) | odor | odorless | | odorless | | |

Units

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