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H2O + KMnO4 + Na2SO3 = KOH + Na2SO4 + Mn2O2

Input interpretation

H_2O water + KMnO_4 potassium permanganate + Na_2SO_3 sodium sulfite ⟶ KOH potassium hydroxide + Na_2SO_4 sodium sulfate + Mn2O2
H_2O water + KMnO_4 potassium permanganate + Na_2SO_3 sodium sulfite ⟶ KOH potassium hydroxide + Na_2SO_4 sodium sulfate + Mn2O2

Balanced equation

Balance the chemical equation algebraically: H_2O + KMnO_4 + Na_2SO_3 ⟶ KOH + Na_2SO_4 + Mn2O2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 Na_2SO_3 ⟶ c_4 KOH + c_5 Na_2SO_4 + c_6 Mn2O2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn, Na and S: H: | 2 c_1 = c_4 O: | c_1 + 4 c_2 + 3 c_3 = c_4 + 4 c_5 + 2 c_6 K: | c_2 = c_4 Mn: | c_2 = 2 c_6 Na: | 2 c_3 = 2 c_5 S: | c_3 = c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 5 c_4 = 2 c_5 = 5 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + 2 KMnO_4 + 5 Na_2SO_3 ⟶ 2 KOH + 5 Na_2SO_4 + Mn2O2
Balance the chemical equation algebraically: H_2O + KMnO_4 + Na_2SO_3 ⟶ KOH + Na_2SO_4 + Mn2O2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 Na_2SO_3 ⟶ c_4 KOH + c_5 Na_2SO_4 + c_6 Mn2O2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn, Na and S: H: | 2 c_1 = c_4 O: | c_1 + 4 c_2 + 3 c_3 = c_4 + 4 c_5 + 2 c_6 K: | c_2 = c_4 Mn: | c_2 = 2 c_6 Na: | 2 c_3 = 2 c_5 S: | c_3 = c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 5 c_4 = 2 c_5 = 5 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + 2 KMnO_4 + 5 Na_2SO_3 ⟶ 2 KOH + 5 Na_2SO_4 + Mn2O2

Structures

+ + ⟶ + + Mn2O2
+ + ⟶ + + Mn2O2

Names

water + potassium permanganate + sodium sulfite ⟶ potassium hydroxide + sodium sulfate + Mn2O2
water + potassium permanganate + sodium sulfite ⟶ potassium hydroxide + sodium sulfate + Mn2O2

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + Na_2SO_3 ⟶ KOH + Na_2SO_4 + Mn2O2 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: H_2O + 2 KMnO_4 + 5 Na_2SO_3 ⟶ 2 KOH + 5 Na_2SO_4 + Mn2O2 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 H_2O | 1 | -1 KMnO_4 | 2 | -2 Na_2SO_3 | 5 | -5 KOH | 2 | 2 Na_2SO_4 | 5 | 5 Mn2O2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) Na_2SO_3 | 5 | -5 | ([Na2SO3])^(-5) KOH | 2 | 2 | ([KOH])^2 Na_2SO_4 | 5 | 5 | ([Na2SO4])^5 Mn2O2 | 1 | 1 | [Mn2O2] 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 = ([H2O])^(-1) ([KMnO4])^(-2) ([Na2SO3])^(-5) ([KOH])^2 ([Na2SO4])^5 [Mn2O2] = (([KOH])^2 ([Na2SO4])^5 [Mn2O2])/([H2O] ([KMnO4])^2 ([Na2SO3])^5)
Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + Na_2SO_3 ⟶ KOH + Na_2SO_4 + Mn2O2 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: H_2O + 2 KMnO_4 + 5 Na_2SO_3 ⟶ 2 KOH + 5 Na_2SO_4 + Mn2O2 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 H_2O | 1 | -1 KMnO_4 | 2 | -2 Na_2SO_3 | 5 | -5 KOH | 2 | 2 Na_2SO_4 | 5 | 5 Mn2O2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) Na_2SO_3 | 5 | -5 | ([Na2SO3])^(-5) KOH | 2 | 2 | ([KOH])^2 Na_2SO_4 | 5 | 5 | ([Na2SO4])^5 Mn2O2 | 1 | 1 | [Mn2O2] 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 = ([H2O])^(-1) ([KMnO4])^(-2) ([Na2SO3])^(-5) ([KOH])^2 ([Na2SO4])^5 [Mn2O2] = (([KOH])^2 ([Na2SO4])^5 [Mn2O2])/([H2O] ([KMnO4])^2 ([Na2SO3])^5)

Rate of reaction

Construct the rate of reaction expression for: H_2O + KMnO_4 + Na_2SO_3 ⟶ KOH + Na_2SO_4 + Mn2O2 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: H_2O + 2 KMnO_4 + 5 Na_2SO_3 ⟶ 2 KOH + 5 Na_2SO_4 + Mn2O2 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 H_2O | 1 | -1 KMnO_4 | 2 | -2 Na_2SO_3 | 5 | -5 KOH | 2 | 2 Na_2SO_4 | 5 | 5 Mn2O2 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) Na_2SO_3 | 5 | -5 | -1/5 (Δ[Na2SO3])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) Na_2SO_4 | 5 | 5 | 1/5 (Δ[Na2SO4])/(Δt) Mn2O2 | 1 | 1 | (Δ[Mn2O2])/(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 = -(Δ[H2O])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/5 (Δ[Na2SO3])/(Δt) = 1/2 (Δ[KOH])/(Δt) = 1/5 (Δ[Na2SO4])/(Δt) = (Δ[Mn2O2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + KMnO_4 + Na_2SO_3 ⟶ KOH + Na_2SO_4 + Mn2O2 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: H_2O + 2 KMnO_4 + 5 Na_2SO_3 ⟶ 2 KOH + 5 Na_2SO_4 + Mn2O2 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 H_2O | 1 | -1 KMnO_4 | 2 | -2 Na_2SO_3 | 5 | -5 KOH | 2 | 2 Na_2SO_4 | 5 | 5 Mn2O2 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) Na_2SO_3 | 5 | -5 | -1/5 (Δ[Na2SO3])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) Na_2SO_4 | 5 | 5 | 1/5 (Δ[Na2SO4])/(Δt) Mn2O2 | 1 | 1 | (Δ[Mn2O2])/(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 = -(Δ[H2O])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/5 (Δ[Na2SO3])/(Δt) = 1/2 (Δ[KOH])/(Δt) = 1/5 (Δ[Na2SO4])/(Δt) = (Δ[Mn2O2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | potassium permanganate | sodium sulfite | potassium hydroxide | sodium sulfate | Mn2O2 formula | H_2O | KMnO_4 | Na_2SO_3 | KOH | Na_2SO_4 | Mn2O2 Hill formula | H_2O | KMnO_4 | Na_2O_3S | HKO | Na_2O_4S | Mn2O2 name | water | potassium permanganate | sodium sulfite | potassium hydroxide | sodium sulfate | IUPAC name | water | potassium permanganate | disodium sulfite | potassium hydroxide | disodium sulfate |
| water | potassium permanganate | sodium sulfite | potassium hydroxide | sodium sulfate | Mn2O2 formula | H_2O | KMnO_4 | Na_2SO_3 | KOH | Na_2SO_4 | Mn2O2 Hill formula | H_2O | KMnO_4 | Na_2O_3S | HKO | Na_2O_4S | Mn2O2 name | water | potassium permanganate | sodium sulfite | potassium hydroxide | sodium sulfate | IUPAC name | water | potassium permanganate | disodium sulfite | potassium hydroxide | disodium sulfate |

Substance properties

| water | potassium permanganate | sodium sulfite | potassium hydroxide | sodium sulfate | Mn2O2 molar mass | 18.015 g/mol | 158.03 g/mol | 126.04 g/mol | 56.105 g/mol | 142.04 g/mol | 141.874 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 0 °C | 240 °C | 500 °C | 406 °C | 884 °C | boiling point | 99.9839 °C | | | 1327 °C | 1429 °C | density | 1 g/cm^3 | 1 g/cm^3 | 2.63 g/cm^3 | 2.044 g/cm^3 | 2.68 g/cm^3 | solubility in water | | | | soluble | soluble | surface tension | 0.0728 N/m | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | 0.001 Pa s (at 550 °C) | | odor | odorless | odorless | | | |
| water | potassium permanganate | sodium sulfite | potassium hydroxide | sodium sulfate | Mn2O2 molar mass | 18.015 g/mol | 158.03 g/mol | 126.04 g/mol | 56.105 g/mol | 142.04 g/mol | 141.874 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 0 °C | 240 °C | 500 °C | 406 °C | 884 °C | boiling point | 99.9839 °C | | | 1327 °C | 1429 °C | density | 1 g/cm^3 | 1 g/cm^3 | 2.63 g/cm^3 | 2.044 g/cm^3 | 2.68 g/cm^3 | solubility in water | | | | soluble | soluble | surface tension | 0.0728 N/m | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | 0.001 Pa s (at 550 °C) | | odor | odorless | odorless | | | |

Units

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