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H2O + KBrO3 + Na2C2O4 = NaOH + CO2 + KBr

Input interpretation

H_2O water + KBrO_3 potassium bromate + Na_2C_2O_4 sodium oxalate ⟶ NaOH sodium hydroxide + CO_2 carbon dioxide + KBr potassium bromide
H_2O water + KBrO_3 potassium bromate + Na_2C_2O_4 sodium oxalate ⟶ NaOH sodium hydroxide + CO_2 carbon dioxide + KBr potassium bromide

Balanced equation

Balance the chemical equation algebraically: H_2O + KBrO_3 + Na_2C_2O_4 ⟶ NaOH + CO_2 + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KBrO_3 + c_3 Na_2C_2O_4 ⟶ c_4 NaOH + c_5 CO_2 + c_6 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Br, K, C and Na: H: | 2 c_1 = c_4 O: | c_1 + 3 c_2 + 4 c_3 = c_4 + 2 c_5 Br: | c_2 = c_6 K: | c_2 = c_6 C: | 2 c_3 = c_5 Na: | 2 c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 6 c_5 = 6 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + KBrO_3 + 3 Na_2C_2O_4 ⟶ 6 NaOH + 6 CO_2 + KBr
Balance the chemical equation algebraically: H_2O + KBrO_3 + Na_2C_2O_4 ⟶ NaOH + CO_2 + KBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KBrO_3 + c_3 Na_2C_2O_4 ⟶ c_4 NaOH + c_5 CO_2 + c_6 KBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Br, K, C and Na: H: | 2 c_1 = c_4 O: | c_1 + 3 c_2 + 4 c_3 = c_4 + 2 c_5 Br: | c_2 = c_6 K: | c_2 = c_6 C: | 2 c_3 = c_5 Na: | 2 c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 6 c_5 = 6 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + KBrO_3 + 3 Na_2C_2O_4 ⟶ 6 NaOH + 6 CO_2 + KBr

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + potassium bromate + sodium oxalate ⟶ sodium hydroxide + carbon dioxide + potassium bromide
water + potassium bromate + sodium oxalate ⟶ sodium hydroxide + carbon dioxide + potassium bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + KBrO_3 + Na_2C_2O_4 ⟶ NaOH + CO_2 + KBr 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: 3 H_2O + KBrO_3 + 3 Na_2C_2O_4 ⟶ 6 NaOH + 6 CO_2 + KBr 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 | 3 | -3 KBrO_3 | 1 | -1 Na_2C_2O_4 | 3 | -3 NaOH | 6 | 6 CO_2 | 6 | 6 KBr | 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 | 3 | -3 | ([H2O])^(-3) KBrO_3 | 1 | -1 | ([KBrO3])^(-1) Na_2C_2O_4 | 3 | -3 | ([Na2C2O4])^(-3) NaOH | 6 | 6 | ([NaOH])^6 CO_2 | 6 | 6 | ([CO2])^6 KBr | 1 | 1 | [KBr] 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])^(-3) ([KBrO3])^(-1) ([Na2C2O4])^(-3) ([NaOH])^6 ([CO2])^6 [KBr] = (([NaOH])^6 ([CO2])^6 [KBr])/(([H2O])^3 [KBrO3] ([Na2C2O4])^3)
Construct the equilibrium constant, K, expression for: H_2O + KBrO_3 + Na_2C_2O_4 ⟶ NaOH + CO_2 + KBr 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: 3 H_2O + KBrO_3 + 3 Na_2C_2O_4 ⟶ 6 NaOH + 6 CO_2 + KBr 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 | 3 | -3 KBrO_3 | 1 | -1 Na_2C_2O_4 | 3 | -3 NaOH | 6 | 6 CO_2 | 6 | 6 KBr | 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 | 3 | -3 | ([H2O])^(-3) KBrO_3 | 1 | -1 | ([KBrO3])^(-1) Na_2C_2O_4 | 3 | -3 | ([Na2C2O4])^(-3) NaOH | 6 | 6 | ([NaOH])^6 CO_2 | 6 | 6 | ([CO2])^6 KBr | 1 | 1 | [KBr] 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])^(-3) ([KBrO3])^(-1) ([Na2C2O4])^(-3) ([NaOH])^6 ([CO2])^6 [KBr] = (([NaOH])^6 ([CO2])^6 [KBr])/(([H2O])^3 [KBrO3] ([Na2C2O4])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2O + KBrO_3 + Na_2C_2O_4 ⟶ NaOH + CO_2 + KBr 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: 3 H_2O + KBrO_3 + 3 Na_2C_2O_4 ⟶ 6 NaOH + 6 CO_2 + KBr 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 | 3 | -3 KBrO_3 | 1 | -1 Na_2C_2O_4 | 3 | -3 NaOH | 6 | 6 CO_2 | 6 | 6 KBr | 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 | 3 | -3 | -1/3 (Δ[H2O])/(Δt) KBrO_3 | 1 | -1 | -(Δ[KBrO3])/(Δt) Na_2C_2O_4 | 3 | -3 | -1/3 (Δ[Na2C2O4])/(Δt) NaOH | 6 | 6 | 1/6 (Δ[NaOH])/(Δt) CO_2 | 6 | 6 | 1/6 (Δ[CO2])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(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 = -1/3 (Δ[H2O])/(Δt) = -(Δ[KBrO3])/(Δt) = -1/3 (Δ[Na2C2O4])/(Δt) = 1/6 (Δ[NaOH])/(Δt) = 1/6 (Δ[CO2])/(Δt) = (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + KBrO_3 + Na_2C_2O_4 ⟶ NaOH + CO_2 + KBr 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: 3 H_2O + KBrO_3 + 3 Na_2C_2O_4 ⟶ 6 NaOH + 6 CO_2 + KBr 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 | 3 | -3 KBrO_3 | 1 | -1 Na_2C_2O_4 | 3 | -3 NaOH | 6 | 6 CO_2 | 6 | 6 KBr | 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 | 3 | -3 | -1/3 (Δ[H2O])/(Δt) KBrO_3 | 1 | -1 | -(Δ[KBrO3])/(Δt) Na_2C_2O_4 | 3 | -3 | -1/3 (Δ[Na2C2O4])/(Δt) NaOH | 6 | 6 | 1/6 (Δ[NaOH])/(Δt) CO_2 | 6 | 6 | 1/6 (Δ[CO2])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(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 = -1/3 (Δ[H2O])/(Δt) = -(Δ[KBrO3])/(Δt) = -1/3 (Δ[Na2C2O4])/(Δt) = 1/6 (Δ[NaOH])/(Δt) = 1/6 (Δ[CO2])/(Δt) = (Δ[KBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | potassium bromate | sodium oxalate | sodium hydroxide | carbon dioxide | potassium bromide formula | H_2O | KBrO_3 | Na_2C_2O_4 | NaOH | CO_2 | KBr Hill formula | H_2O | BrKO_3 | Na_2C_2O_4 | HNaO | CO_2 | BrK name | water | potassium bromate | sodium oxalate | sodium hydroxide | carbon dioxide | potassium bromide IUPAC name | water | potassium bromate | disodium oxalate | sodium hydroxide | carbon dioxide | potassium bromide
| water | potassium bromate | sodium oxalate | sodium hydroxide | carbon dioxide | potassium bromide formula | H_2O | KBrO_3 | Na_2C_2O_4 | NaOH | CO_2 | KBr Hill formula | H_2O | BrKO_3 | Na_2C_2O_4 | HNaO | CO_2 | BrK name | water | potassium bromate | sodium oxalate | sodium hydroxide | carbon dioxide | potassium bromide IUPAC name | water | potassium bromate | disodium oxalate | sodium hydroxide | carbon dioxide | potassium bromide

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