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KOH + H3PO3 + KClO2 = H2O + KCl + K3PO4

Input interpretation

KOH potassium hydroxide + HP(O)(OH)_2 phosphorous acid + KClO2 ⟶ H_2O water + KCl potassium chloride + K3PO4
KOH potassium hydroxide + HP(O)(OH)_2 phosphorous acid + KClO2 ⟶ H_2O water + KCl potassium chloride + K3PO4

Balanced equation

Balance the chemical equation algebraically: KOH + HP(O)(OH)_2 + KClO2 ⟶ H_2O + KCl + K3PO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 HP(O)(OH)_2 + c_3 KClO2 ⟶ c_4 H_2O + c_5 KCl + c_6 K3PO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, P and Cl: H: | c_1 + 3 c_2 = 2 c_4 K: | c_1 + c_3 = c_5 + 3 c_6 O: | c_1 + 3 c_2 + 2 c_3 = c_4 + 4 c_6 P: | c_2 = c_6 Cl: | 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 = 6 c_2 = 2 c_3 = 1 c_4 = 6 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KOH + 2 HP(O)(OH)_2 + KClO2 ⟶ 6 H_2O + KCl + 2 K3PO4
Balance the chemical equation algebraically: KOH + HP(O)(OH)_2 + KClO2 ⟶ H_2O + KCl + K3PO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 HP(O)(OH)_2 + c_3 KClO2 ⟶ c_4 H_2O + c_5 KCl + c_6 K3PO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, P and Cl: H: | c_1 + 3 c_2 = 2 c_4 K: | c_1 + c_3 = c_5 + 3 c_6 O: | c_1 + 3 c_2 + 2 c_3 = c_4 + 4 c_6 P: | c_2 = c_6 Cl: | 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 = 6 c_2 = 2 c_3 = 1 c_4 = 6 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 KOH + 2 HP(O)(OH)_2 + KClO2 ⟶ 6 H_2O + KCl + 2 K3PO4

Structures

+ + KClO2 ⟶ + + K3PO4
+ + KClO2 ⟶ + + K3PO4

Names

potassium hydroxide + phosphorous acid + KClO2 ⟶ water + potassium chloride + K3PO4
potassium hydroxide + phosphorous acid + KClO2 ⟶ water + potassium chloride + K3PO4

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + HP(O)(OH)_2 + KClO2 ⟶ H_2O + KCl + K3PO4 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 + 2 HP(O)(OH)_2 + KClO2 ⟶ 6 H_2O + KCl + 2 K3PO4 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 HP(O)(OH)_2 | 2 | -2 KClO2 | 1 | -1 H_2O | 6 | 6 KCl | 1 | 1 K3PO4 | 2 | 2 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) HP(O)(OH)_2 | 2 | -2 | ([HP(O)(OH)2])^(-2) KClO2 | 1 | -1 | ([KClO2])^(-1) H_2O | 6 | 6 | ([H2O])^6 KCl | 1 | 1 | [KCl] K3PO4 | 2 | 2 | ([K3PO4])^2 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) ([HP(O)(OH)2])^(-2) ([KClO2])^(-1) ([H2O])^6 [KCl] ([K3PO4])^2 = (([H2O])^6 [KCl] ([K3PO4])^2)/(([KOH])^6 ([HP(O)(OH)2])^2 [KClO2])
Construct the equilibrium constant, K, expression for: KOH + HP(O)(OH)_2 + KClO2 ⟶ H_2O + KCl + K3PO4 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 + 2 HP(O)(OH)_2 + KClO2 ⟶ 6 H_2O + KCl + 2 K3PO4 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 HP(O)(OH)_2 | 2 | -2 KClO2 | 1 | -1 H_2O | 6 | 6 KCl | 1 | 1 K3PO4 | 2 | 2 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) HP(O)(OH)_2 | 2 | -2 | ([HP(O)(OH)2])^(-2) KClO2 | 1 | -1 | ([KClO2])^(-1) H_2O | 6 | 6 | ([H2O])^6 KCl | 1 | 1 | [KCl] K3PO4 | 2 | 2 | ([K3PO4])^2 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) ([HP(O)(OH)2])^(-2) ([KClO2])^(-1) ([H2O])^6 [KCl] ([K3PO4])^2 = (([H2O])^6 [KCl] ([K3PO4])^2)/(([KOH])^6 ([HP(O)(OH)2])^2 [KClO2])

Rate of reaction

Construct the rate of reaction expression for: KOH + HP(O)(OH)_2 + KClO2 ⟶ H_2O + KCl + K3PO4 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 + 2 HP(O)(OH)_2 + KClO2 ⟶ 6 H_2O + KCl + 2 K3PO4 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 HP(O)(OH)_2 | 2 | -2 KClO2 | 1 | -1 H_2O | 6 | 6 KCl | 1 | 1 K3PO4 | 2 | 2 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) HP(O)(OH)_2 | 2 | -2 | -1/2 (Δ[HP(O)(OH)2])/(Δt) KClO2 | 1 | -1 | -(Δ[KClO2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) K3PO4 | 2 | 2 | 1/2 (Δ[K3PO4])/(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) = -1/2 (Δ[HP(O)(OH)2])/(Δt) = -(Δ[KClO2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[K3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + HP(O)(OH)_2 + KClO2 ⟶ H_2O + KCl + K3PO4 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 + 2 HP(O)(OH)_2 + KClO2 ⟶ 6 H_2O + KCl + 2 K3PO4 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 HP(O)(OH)_2 | 2 | -2 KClO2 | 1 | -1 H_2O | 6 | 6 KCl | 1 | 1 K3PO4 | 2 | 2 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) HP(O)(OH)_2 | 2 | -2 | -1/2 (Δ[HP(O)(OH)2])/(Δt) KClO2 | 1 | -1 | -(Δ[KClO2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) K3PO4 | 2 | 2 | 1/2 (Δ[K3PO4])/(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) = -1/2 (Δ[HP(O)(OH)2])/(Δt) = -(Δ[KClO2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[K3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | phosphorous acid | KClO2 | water | potassium chloride | K3PO4 formula | KOH | HP(O)(OH)_2 | KClO2 | H_2O | KCl | K3PO4 Hill formula | HKO | H_3O_3P | ClKO2 | H_2O | ClK | K3O4P name | potassium hydroxide | phosphorous acid | | water | potassium chloride |
| potassium hydroxide | phosphorous acid | KClO2 | water | potassium chloride | K3PO4 formula | KOH | HP(O)(OH)_2 | KClO2 | H_2O | KCl | K3PO4 Hill formula | HKO | H_3O_3P | ClKO2 | H_2O | ClK | K3O4P name | potassium hydroxide | phosphorous acid | | water | potassium chloride |

Substance properties

| potassium hydroxide | phosphorous acid | KClO2 | water | potassium chloride | K3PO4 molar mass | 56.105 g/mol | 81.995 g/mol | 106.5 g/mol | 18.015 g/mol | 74.55 g/mol | 212.26 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | melting point | 406 °C | 74 °C | | 0 °C | 770 °C | boiling point | 1327 °C | | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | 1.597 g/cm^3 | | 1 g/cm^3 | 1.98 g/cm^3 | solubility in water | soluble | | | | soluble | 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 | phosphorous acid | KClO2 | water | potassium chloride | K3PO4 molar mass | 56.105 g/mol | 81.995 g/mol | 106.5 g/mol | 18.015 g/mol | 74.55 g/mol | 212.26 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | melting point | 406 °C | 74 °C | | 0 °C | 770 °C | boiling point | 1327 °C | | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | 1.597 g/cm^3 | | 1 g/cm^3 | 1.98 g/cm^3 | solubility in water | soluble | | | | soluble | 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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