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KOH + KNO3 + NMnO2 = H2O + K2MnO4 + KNO2

Input interpretation

KOH potassium hydroxide + KNO_3 potassium nitrate + NMnO2 ⟶ H_2O water + K_2MnO_4 potassium manganate + KNO_2 potassium nitrite
KOH potassium hydroxide + KNO_3 potassium nitrate + NMnO2 ⟶ H_2O water + K_2MnO_4 potassium manganate + KNO_2 potassium nitrite

Balanced equation

Balance the chemical equation algebraically: KOH + KNO_3 + NMnO2 ⟶ H_2O + K_2MnO_4 + KNO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KNO_3 + c_3 NMnO2 ⟶ c_4 H_2O + c_5 K_2MnO_4 + c_6 KNO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, N and Mn: H: | c_1 = 2 c_4 K: | c_1 + c_2 = 2 c_5 + c_6 O: | c_1 + 3 c_2 + 2 c_3 = c_4 + 4 c_5 + 2 c_6 N: | c_2 + c_3 = c_6 Mn: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 5/2 c_3 = 1 c_4 = 3/2 c_5 = 1 c_6 = 7/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 5 c_3 = 2 c_4 = 3 c_5 = 2 c_6 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KOH + 5 KNO_3 + 2 NMnO2 ⟶ 3 H_2O + 2 K_2MnO_4 + 7 KNO_2
Balance the chemical equation algebraically: KOH + KNO_3 + NMnO2 ⟶ H_2O + K_2MnO_4 + KNO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 KNO_3 + c_3 NMnO2 ⟶ c_4 H_2O + c_5 K_2MnO_4 + c_6 KNO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, N and Mn: H: | c_1 = 2 c_4 K: | c_1 + c_2 = 2 c_5 + c_6 O: | c_1 + 3 c_2 + 2 c_3 = c_4 + 4 c_5 + 2 c_6 N: | c_2 + c_3 = c_6 Mn: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 5/2 c_3 = 1 c_4 = 3/2 c_5 = 1 c_6 = 7/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 5 c_3 = 2 c_4 = 3 c_5 = 2 c_6 = 7 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KOH + 5 KNO_3 + 2 NMnO2 ⟶ 3 H_2O + 2 K_2MnO_4 + 7 KNO_2

Structures

+ + NMnO2 ⟶ + +
+ + NMnO2 ⟶ + +

Names

potassium hydroxide + potassium nitrate + NMnO2 ⟶ water + potassium manganate + potassium nitrite
potassium hydroxide + potassium nitrate + NMnO2 ⟶ water + potassium manganate + potassium nitrite

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + KNO_3 + NMnO2 ⟶ H_2O + K_2MnO_4 + KNO_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: 6 KOH + 5 KNO_3 + 2 NMnO2 ⟶ 3 H_2O + 2 K_2MnO_4 + 7 KNO_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 KOH | 6 | -6 KNO_3 | 5 | -5 NMnO2 | 2 | -2 H_2O | 3 | 3 K_2MnO_4 | 2 | 2 KNO_2 | 7 | 7 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 6 | -6 | ([KOH])^(-6) KNO_3 | 5 | -5 | ([KNO3])^(-5) NMnO2 | 2 | -2 | ([NMnO2])^(-2) H_2O | 3 | 3 | ([H2O])^3 K_2MnO_4 | 2 | 2 | ([K2MnO4])^2 KNO_2 | 7 | 7 | ([KNO2])^7 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])^(-6) ([KNO3])^(-5) ([NMnO2])^(-2) ([H2O])^3 ([K2MnO4])^2 ([KNO2])^7 = (([H2O])^3 ([K2MnO4])^2 ([KNO2])^7)/(([KOH])^6 ([KNO3])^5 ([NMnO2])^2)
Construct the equilibrium constant, K, expression for: KOH + KNO_3 + NMnO2 ⟶ H_2O + K_2MnO_4 + KNO_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: 6 KOH + 5 KNO_3 + 2 NMnO2 ⟶ 3 H_2O + 2 K_2MnO_4 + 7 KNO_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 KOH | 6 | -6 KNO_3 | 5 | -5 NMnO2 | 2 | -2 H_2O | 3 | 3 K_2MnO_4 | 2 | 2 KNO_2 | 7 | 7 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 6 | -6 | ([KOH])^(-6) KNO_3 | 5 | -5 | ([KNO3])^(-5) NMnO2 | 2 | -2 | ([NMnO2])^(-2) H_2O | 3 | 3 | ([H2O])^3 K_2MnO_4 | 2 | 2 | ([K2MnO4])^2 KNO_2 | 7 | 7 | ([KNO2])^7 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])^(-6) ([KNO3])^(-5) ([NMnO2])^(-2) ([H2O])^3 ([K2MnO4])^2 ([KNO2])^7 = (([H2O])^3 ([K2MnO4])^2 ([KNO2])^7)/(([KOH])^6 ([KNO3])^5 ([NMnO2])^2)

Rate of reaction

Construct the rate of reaction expression for: KOH + KNO_3 + NMnO2 ⟶ H_2O + K_2MnO_4 + KNO_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: 6 KOH + 5 KNO_3 + 2 NMnO2 ⟶ 3 H_2O + 2 K_2MnO_4 + 7 KNO_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 KOH | 6 | -6 KNO_3 | 5 | -5 NMnO2 | 2 | -2 H_2O | 3 | 3 K_2MnO_4 | 2 | 2 KNO_2 | 7 | 7 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 | 6 | -6 | -1/6 (Δ[KOH])/(Δt) KNO_3 | 5 | -5 | -1/5 (Δ[KNO3])/(Δt) NMnO2 | 2 | -2 | -1/2 (Δ[NMnO2])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2MnO_4 | 2 | 2 | 1/2 (Δ[K2MnO4])/(Δt) KNO_2 | 7 | 7 | 1/7 (Δ[KNO2])/(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 = -1/6 (Δ[KOH])/(Δt) = -1/5 (Δ[KNO3])/(Δt) = -1/2 (Δ[NMnO2])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[K2MnO4])/(Δt) = 1/7 (Δ[KNO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + KNO_3 + NMnO2 ⟶ H_2O + K_2MnO_4 + KNO_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: 6 KOH + 5 KNO_3 + 2 NMnO2 ⟶ 3 H_2O + 2 K_2MnO_4 + 7 KNO_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 KOH | 6 | -6 KNO_3 | 5 | -5 NMnO2 | 2 | -2 H_2O | 3 | 3 K_2MnO_4 | 2 | 2 KNO_2 | 7 | 7 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 | 6 | -6 | -1/6 (Δ[KOH])/(Δt) KNO_3 | 5 | -5 | -1/5 (Δ[KNO3])/(Δt) NMnO2 | 2 | -2 | -1/2 (Δ[NMnO2])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2MnO_4 | 2 | 2 | 1/2 (Δ[K2MnO4])/(Δt) KNO_2 | 7 | 7 | 1/7 (Δ[KNO2])/(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 = -1/6 (Δ[KOH])/(Δt) = -1/5 (Δ[KNO3])/(Δt) = -1/2 (Δ[NMnO2])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[K2MnO4])/(Δt) = 1/7 (Δ[KNO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | potassium nitrate | NMnO2 | water | potassium manganate | potassium nitrite formula | KOH | KNO_3 | NMnO2 | H_2O | K_2MnO_4 | KNO_2 Hill formula | HKO | KNO_3 | MnNO2 | H_2O | K_2MnO_4 | KNO_2 name | potassium hydroxide | potassium nitrate | | water | potassium manganate | potassium nitrite IUPAC name | potassium hydroxide | potassium nitrate | | water | dipotassium dioxido-dioxomanganese | potassium nitrite
| potassium hydroxide | potassium nitrate | NMnO2 | water | potassium manganate | potassium nitrite formula | KOH | KNO_3 | NMnO2 | H_2O | K_2MnO_4 | KNO_2 Hill formula | HKO | KNO_3 | MnNO2 | H_2O | K_2MnO_4 | KNO_2 name | potassium hydroxide | potassium nitrate | | water | potassium manganate | potassium nitrite IUPAC name | potassium hydroxide | potassium nitrate | | water | dipotassium dioxido-dioxomanganese | potassium nitrite

Substance properties

| potassium hydroxide | potassium nitrate | NMnO2 | water | potassium manganate | potassium nitrite molar mass | 56.105 g/mol | 101.1 g/mol | 100.94 g/mol | 18.015 g/mol | 197.13 g/mol | 85.103 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | 334 °C | | 0 °C | 190 °C | 350 °C boiling point | 1327 °C | | | 99.9839 °C | | density | 2.044 g/cm^3 | | | 1 g/cm^3 | | 1.915 g/cm^3 solubility in water | soluble | soluble | | | decomposes | surface tension | | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | odorless | | odorless | |
| potassium hydroxide | potassium nitrate | NMnO2 | water | potassium manganate | potassium nitrite molar mass | 56.105 g/mol | 101.1 g/mol | 100.94 g/mol | 18.015 g/mol | 197.13 g/mol | 85.103 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | 334 °C | | 0 °C | 190 °C | 350 °C boiling point | 1327 °C | | | 99.9839 °C | | density | 2.044 g/cm^3 | | | 1 g/cm^3 | | 1.915 g/cm^3 solubility in water | soluble | soluble | | | decomposes | surface tension | | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | odorless | | odorless | |

Units

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