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NaOH + MnO2 + KNO3 = H2O + KNO2 + Na2MnO4

Input interpretation

NaOH sodium hydroxide + MnO_2 manganese dioxide + KNO_3 potassium nitrate ⟶ H_2O water + KNO_2 potassium nitrite + Na2MnO4
NaOH sodium hydroxide + MnO_2 manganese dioxide + KNO_3 potassium nitrate ⟶ H_2O water + KNO_2 potassium nitrite + Na2MnO4

Balanced equation

Balance the chemical equation algebraically: NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 MnO_2 + c_3 KNO_3 ⟶ c_4 H_2O + c_5 KNO_2 + c_6 Na2MnO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Mn, K and N: H: | c_1 = 2 c_4 Na: | c_1 = 2 c_6 O: | c_1 + 2 c_2 + 3 c_3 = c_4 + 2 c_5 + 4 c_6 Mn: | c_2 = c_6 K: | c_3 = c_5 N: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4
Balance the chemical equation algebraically: NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 MnO_2 + c_3 KNO_3 ⟶ c_4 H_2O + c_5 KNO_2 + c_6 Na2MnO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Mn, K and N: H: | c_1 = 2 c_4 Na: | c_1 = 2 c_6 O: | c_1 + 2 c_2 + 3 c_3 = c_4 + 2 c_5 + 4 c_6 Mn: | c_2 = c_6 K: | c_3 = c_5 N: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4

Structures

+ + ⟶ + + Na2MnO4
+ + ⟶ + + Na2MnO4

Names

sodium hydroxide + manganese dioxide + potassium nitrate ⟶ water + potassium nitrite + Na2MnO4
sodium hydroxide + manganese dioxide + potassium nitrate ⟶ water + potassium nitrite + Na2MnO4

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH | 2 | -2 MnO_2 | 1 | -1 KNO_3 | 1 | -1 H_2O | 1 | 1 KNO_2 | 1 | 1 Na2MnO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) MnO_2 | 1 | -1 | ([MnO2])^(-1) KNO_3 | 1 | -1 | ([KNO3])^(-1) H_2O | 1 | 1 | [H2O] KNO_2 | 1 | 1 | [KNO2] Na2MnO4 | 1 | 1 | [Na2MnO4] 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 = ([NaOH])^(-2) ([MnO2])^(-1) ([KNO3])^(-1) [H2O] [KNO2] [Na2MnO4] = ([H2O] [KNO2] [Na2MnO4])/(([NaOH])^2 [MnO2] [KNO3])
Construct the equilibrium constant, K, expression for: NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH | 2 | -2 MnO_2 | 1 | -1 KNO_3 | 1 | -1 H_2O | 1 | 1 KNO_2 | 1 | 1 Na2MnO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) MnO_2 | 1 | -1 | ([MnO2])^(-1) KNO_3 | 1 | -1 | ([KNO3])^(-1) H_2O | 1 | 1 | [H2O] KNO_2 | 1 | 1 | [KNO2] Na2MnO4 | 1 | 1 | [Na2MnO4] 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 = ([NaOH])^(-2) ([MnO2])^(-1) ([KNO3])^(-1) [H2O] [KNO2] [Na2MnO4] = ([H2O] [KNO2] [Na2MnO4])/(([NaOH])^2 [MnO2] [KNO3])

Rate of reaction

Construct the rate of reaction expression for: NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH | 2 | -2 MnO_2 | 1 | -1 KNO_3 | 1 | -1 H_2O | 1 | 1 KNO_2 | 1 | 1 Na2MnO4 | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) KNO_3 | 1 | -1 | -(Δ[KNO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KNO_2 | 1 | 1 | (Δ[KNO2])/(Δt) Na2MnO4 | 1 | 1 | (Δ[Na2MnO4])/(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[NaOH])/(Δt) = -(Δ[MnO2])/(Δt) = -(Δ[KNO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KNO2])/(Δt) = (Δ[Na2MnO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH + MnO_2 + KNO_3 ⟶ H_2O + KNO_2 + Na2MnO4 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 NaOH | 2 | -2 MnO_2 | 1 | -1 KNO_3 | 1 | -1 H_2O | 1 | 1 KNO_2 | 1 | 1 Na2MnO4 | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) KNO_3 | 1 | -1 | -(Δ[KNO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KNO_2 | 1 | 1 | (Δ[KNO2])/(Δt) Na2MnO4 | 1 | 1 | (Δ[Na2MnO4])/(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[NaOH])/(Δt) = -(Δ[MnO2])/(Δt) = -(Δ[KNO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KNO2])/(Δt) = (Δ[Na2MnO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | manganese dioxide | potassium nitrate | water | potassium nitrite | Na2MnO4 formula | NaOH | MnO_2 | KNO_3 | H_2O | KNO_2 | Na2MnO4 Hill formula | HNaO | MnO_2 | KNO_3 | H_2O | KNO_2 | MnNa2O4 name | sodium hydroxide | manganese dioxide | potassium nitrate | water | potassium nitrite | IUPAC name | sodium hydroxide | dioxomanganese | potassium nitrate | water | potassium nitrite |
| sodium hydroxide | manganese dioxide | potassium nitrate | water | potassium nitrite | Na2MnO4 formula | NaOH | MnO_2 | KNO_3 | H_2O | KNO_2 | Na2MnO4 Hill formula | HNaO | MnO_2 | KNO_3 | H_2O | KNO_2 | MnNa2O4 name | sodium hydroxide | manganese dioxide | potassium nitrate | water | potassium nitrite | IUPAC name | sodium hydroxide | dioxomanganese | potassium nitrate | water | potassium nitrite |

Substance properties

| sodium hydroxide | manganese dioxide | potassium nitrate | water | potassium nitrite | Na2MnO4 molar mass | 39.997 g/mol | 86.936 g/mol | 101.1 g/mol | 18.015 g/mol | 85.103 g/mol | 164.91 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 323 °C | 535 °C | 334 °C | 0 °C | 350 °C | boiling point | 1390 °C | | | 99.9839 °C | | density | 2.13 g/cm^3 | 5.03 g/cm^3 | | 1 g/cm^3 | 1.915 g/cm^3 | solubility in water | soluble | insoluble | soluble | | | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless | |
| sodium hydroxide | manganese dioxide | potassium nitrate | water | potassium nitrite | Na2MnO4 molar mass | 39.997 g/mol | 86.936 g/mol | 101.1 g/mol | 18.015 g/mol | 85.103 g/mol | 164.91 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 323 °C | 535 °C | 334 °C | 0 °C | 350 °C | boiling point | 1390 °C | | | 99.9839 °C | | density | 2.13 g/cm^3 | 5.03 g/cm^3 | | 1 g/cm^3 | 1.915 g/cm^3 | solubility in water | soluble | insoluble | soluble | | | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless | |

Units

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