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HCl + KBr + NaClO3 = H2O + NaCl + KCl + Br2

Input interpretation

HCl hydrogen chloride + KBr potassium bromide + NaClO_3 sodium chlorate ⟶ H_2O water + NaCl sodium chloride + KCl potassium chloride + Br_2 bromine
HCl hydrogen chloride + KBr potassium bromide + NaClO_3 sodium chlorate ⟶ H_2O water + NaCl sodium chloride + KCl potassium chloride + Br_2 bromine

Balanced equation

Balance the chemical equation algebraically: HCl + KBr + NaClO_3 ⟶ H_2O + NaCl + KCl + Br_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KBr + c_3 NaClO_3 ⟶ c_4 H_2O + c_5 NaCl + c_6 KCl + c_7 Br_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Br, K, Na and O: Cl: | c_1 + c_3 = c_5 + c_6 H: | c_1 = 2 c_4 Br: | c_2 = 2 c_7 K: | c_2 = c_6 Na: | c_3 = c_5 O: | 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 1 c_6 = 6 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 6 KBr + NaClO_3 ⟶ 3 H_2O + NaCl + 6 KCl + 3 Br_2
Balance the chemical equation algebraically: HCl + KBr + NaClO_3 ⟶ H_2O + NaCl + KCl + Br_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KBr + c_3 NaClO_3 ⟶ c_4 H_2O + c_5 NaCl + c_6 KCl + c_7 Br_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Br, K, Na and O: Cl: | c_1 + c_3 = c_5 + c_6 H: | c_1 = 2 c_4 Br: | c_2 = 2 c_7 K: | c_2 = c_6 Na: | c_3 = c_5 O: | 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 1 c_6 = 6 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 6 KBr + NaClO_3 ⟶ 3 H_2O + NaCl + 6 KCl + 3 Br_2

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

hydrogen chloride + potassium bromide + sodium chlorate ⟶ water + sodium chloride + potassium chloride + bromine
hydrogen chloride + potassium bromide + sodium chlorate ⟶ water + sodium chloride + potassium chloride + bromine

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + KBr + NaClO_3 ⟶ H_2O + NaCl + KCl + Br_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 HCl + 6 KBr + NaClO_3 ⟶ 3 H_2O + NaCl + 6 KCl + 3 Br_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 HCl | 6 | -6 KBr | 6 | -6 NaClO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 1 | 1 KCl | 6 | 6 Br_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) KBr | 6 | -6 | ([KBr])^(-6) NaClO_3 | 1 | -1 | ([NaClO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 NaCl | 1 | 1 | [NaCl] KCl | 6 | 6 | ([KCl])^6 Br_2 | 3 | 3 | ([Br2])^3 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 = ([HCl])^(-6) ([KBr])^(-6) ([NaClO3])^(-1) ([H2O])^3 [NaCl] ([KCl])^6 ([Br2])^3 = (([H2O])^3 [NaCl] ([KCl])^6 ([Br2])^3)/(([HCl])^6 ([KBr])^6 [NaClO3])
Construct the equilibrium constant, K, expression for: HCl + KBr + NaClO_3 ⟶ H_2O + NaCl + KCl + Br_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 HCl + 6 KBr + NaClO_3 ⟶ 3 H_2O + NaCl + 6 KCl + 3 Br_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 HCl | 6 | -6 KBr | 6 | -6 NaClO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 1 | 1 KCl | 6 | 6 Br_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) KBr | 6 | -6 | ([KBr])^(-6) NaClO_3 | 1 | -1 | ([NaClO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 NaCl | 1 | 1 | [NaCl] KCl | 6 | 6 | ([KCl])^6 Br_2 | 3 | 3 | ([Br2])^3 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 = ([HCl])^(-6) ([KBr])^(-6) ([NaClO3])^(-1) ([H2O])^3 [NaCl] ([KCl])^6 ([Br2])^3 = (([H2O])^3 [NaCl] ([KCl])^6 ([Br2])^3)/(([HCl])^6 ([KBr])^6 [NaClO3])

Rate of reaction

Construct the rate of reaction expression for: HCl + KBr + NaClO_3 ⟶ H_2O + NaCl + KCl + Br_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 HCl + 6 KBr + NaClO_3 ⟶ 3 H_2O + NaCl + 6 KCl + 3 Br_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 HCl | 6 | -6 KBr | 6 | -6 NaClO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 1 | 1 KCl | 6 | 6 Br_2 | 3 | 3 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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) KBr | 6 | -6 | -1/6 (Δ[KBr])/(Δt) NaClO_3 | 1 | -1 | -(Δ[NaClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) Br_2 | 3 | 3 | 1/3 (Δ[Br2])/(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[HCl])/(Δt) = -1/6 (Δ[KBr])/(Δt) = -(Δ[NaClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[NaCl])/(Δt) = 1/6 (Δ[KCl])/(Δt) = 1/3 (Δ[Br2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + KBr + NaClO_3 ⟶ H_2O + NaCl + KCl + Br_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 HCl + 6 KBr + NaClO_3 ⟶ 3 H_2O + NaCl + 6 KCl + 3 Br_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 HCl | 6 | -6 KBr | 6 | -6 NaClO_3 | 1 | -1 H_2O | 3 | 3 NaCl | 1 | 1 KCl | 6 | 6 Br_2 | 3 | 3 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 HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) KBr | 6 | -6 | -1/6 (Δ[KBr])/(Δt) NaClO_3 | 1 | -1 | -(Δ[NaClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) KCl | 6 | 6 | 1/6 (Δ[KCl])/(Δt) Br_2 | 3 | 3 | 1/3 (Δ[Br2])/(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[HCl])/(Δt) = -1/6 (Δ[KBr])/(Δt) = -(Δ[NaClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[NaCl])/(Δt) = 1/6 (Δ[KCl])/(Δt) = 1/3 (Δ[Br2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | potassium bromide | sodium chlorate | water | sodium chloride | potassium chloride | bromine formula | HCl | KBr | NaClO_3 | H_2O | NaCl | KCl | Br_2 Hill formula | ClH | BrK | ClNaO_3 | H_2O | ClNa | ClK | Br_2 name | hydrogen chloride | potassium bromide | sodium chlorate | water | sodium chloride | potassium chloride | bromine IUPAC name | hydrogen chloride | potassium bromide | sodium chlorate | water | sodium chloride | potassium chloride | molecular bromine
| hydrogen chloride | potassium bromide | sodium chlorate | water | sodium chloride | potassium chloride | bromine formula | HCl | KBr | NaClO_3 | H_2O | NaCl | KCl | Br_2 Hill formula | ClH | BrK | ClNaO_3 | H_2O | ClNa | ClK | Br_2 name | hydrogen chloride | potassium bromide | sodium chlorate | water | sodium chloride | potassium chloride | bromine IUPAC name | hydrogen chloride | potassium bromide | sodium chlorate | water | sodium chloride | potassium chloride | molecular bromine

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