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HBr + HClO3 = H2O + Cl2 + Br2

Input interpretation

HBr hydrogen bromide + HClO3 ⟶ H_2O water + Cl_2 chlorine + Br_2 bromine
HBr hydrogen bromide + HClO3 ⟶ H_2O water + Cl_2 chlorine + Br_2 bromine

Balanced equation

Balance the chemical equation algebraically: HBr + HClO3 ⟶ H_2O + Cl_2 + Br_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HBr + c_2 HClO3 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 Br_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Br, H, Cl and O: Br: | c_1 = 2 c_5 H: | c_1 + c_2 = 2 c_3 Cl: | c_2 = 2 c_4 O: | 3 c_2 = c_3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 2 c_3 = 6 c_4 = 1 c_5 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HBr + 2 HClO3 ⟶ 6 H_2O + Cl_2 + 5 Br_2
Balance the chemical equation algebraically: HBr + HClO3 ⟶ H_2O + Cl_2 + Br_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HBr + c_2 HClO3 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 Br_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Br, H, Cl and O: Br: | c_1 = 2 c_5 H: | c_1 + c_2 = 2 c_3 Cl: | c_2 = 2 c_4 O: | 3 c_2 = c_3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 2 c_3 = 6 c_4 = 1 c_5 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HBr + 2 HClO3 ⟶ 6 H_2O + Cl_2 + 5 Br_2

Structures

+ HClO3 ⟶ + +
+ HClO3 ⟶ + +

Names

hydrogen bromide + HClO3 ⟶ water + chlorine + bromine
hydrogen bromide + HClO3 ⟶ water + chlorine + bromine

Equilibrium constant

Construct the equilibrium constant, K, expression for: HBr + HClO3 ⟶ H_2O + Cl_2 + 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: 10 HBr + 2 HClO3 ⟶ 6 H_2O + Cl_2 + 5 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 HBr | 10 | -10 HClO3 | 2 | -2 H_2O | 6 | 6 Cl_2 | 1 | 1 Br_2 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HBr | 10 | -10 | ([HBr])^(-10) HClO3 | 2 | -2 | ([HClO3])^(-2) H_2O | 6 | 6 | ([H2O])^6 Cl_2 | 1 | 1 | [Cl2] Br_2 | 5 | 5 | ([Br2])^5 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 = ([HBr])^(-10) ([HClO3])^(-2) ([H2O])^6 [Cl2] ([Br2])^5 = (([H2O])^6 [Cl2] ([Br2])^5)/(([HBr])^10 ([HClO3])^2)
Construct the equilibrium constant, K, expression for: HBr + HClO3 ⟶ H_2O + Cl_2 + 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: 10 HBr + 2 HClO3 ⟶ 6 H_2O + Cl_2 + 5 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 HBr | 10 | -10 HClO3 | 2 | -2 H_2O | 6 | 6 Cl_2 | 1 | 1 Br_2 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HBr | 10 | -10 | ([HBr])^(-10) HClO3 | 2 | -2 | ([HClO3])^(-2) H_2O | 6 | 6 | ([H2O])^6 Cl_2 | 1 | 1 | [Cl2] Br_2 | 5 | 5 | ([Br2])^5 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 = ([HBr])^(-10) ([HClO3])^(-2) ([H2O])^6 [Cl2] ([Br2])^5 = (([H2O])^6 [Cl2] ([Br2])^5)/(([HBr])^10 ([HClO3])^2)

Rate of reaction

Construct the rate of reaction expression for: HBr + HClO3 ⟶ H_2O + Cl_2 + 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: 10 HBr + 2 HClO3 ⟶ 6 H_2O + Cl_2 + 5 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 HBr | 10 | -10 HClO3 | 2 | -2 H_2O | 6 | 6 Cl_2 | 1 | 1 Br_2 | 5 | 5 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 HBr | 10 | -10 | -1/10 (Δ[HBr])/(Δt) HClO3 | 2 | -2 | -1/2 (Δ[HClO3])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) Br_2 | 5 | 5 | 1/5 (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 = -1/10 (Δ[HBr])/(Δt) = -1/2 (Δ[HClO3])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = 1/5 (Δ[Br2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HBr + HClO3 ⟶ H_2O + Cl_2 + 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: 10 HBr + 2 HClO3 ⟶ 6 H_2O + Cl_2 + 5 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 HBr | 10 | -10 HClO3 | 2 | -2 H_2O | 6 | 6 Cl_2 | 1 | 1 Br_2 | 5 | 5 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 HBr | 10 | -10 | -1/10 (Δ[HBr])/(Δt) HClO3 | 2 | -2 | -1/2 (Δ[HClO3])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) Br_2 | 5 | 5 | 1/5 (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 = -1/10 (Δ[HBr])/(Δt) = -1/2 (Δ[HClO3])/(Δt) = 1/6 (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = 1/5 (Δ[Br2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen bromide | HClO3 | water | chlorine | bromine formula | HBr | HClO3 | H_2O | Cl_2 | Br_2 Hill formula | BrH | HClO3 | H_2O | Cl_2 | Br_2 name | hydrogen bromide | | water | chlorine | bromine IUPAC name | hydrogen bromide | | water | molecular chlorine | molecular bromine
| hydrogen bromide | HClO3 | water | chlorine | bromine formula | HBr | HClO3 | H_2O | Cl_2 | Br_2 Hill formula | BrH | HClO3 | H_2O | Cl_2 | Br_2 name | hydrogen bromide | | water | chlorine | bromine IUPAC name | hydrogen bromide | | water | molecular chlorine | molecular bromine

Substance properties

| hydrogen bromide | HClO3 | water | chlorine | bromine molar mass | 80.912 g/mol | 84.45 g/mol | 18.015 g/mol | 70.9 g/mol | 159.81 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | -86.8 °C | | 0 °C | -101 °C | -7.2 °C boiling point | -66.38 °C | | 99.9839 °C | -34 °C | 58.8 °C density | 0.003307 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 3.119 g/cm^3 solubility in water | miscible | | | | insoluble surface tension | 0.0271 N/m | | 0.0728 N/m | | 0.0409 N/m dynamic viscosity | 8.4×10^-4 Pa s (at -75 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 9.44×10^-4 Pa s (at 25 °C) odor | | | odorless | |
| hydrogen bromide | HClO3 | water | chlorine | bromine molar mass | 80.912 g/mol | 84.45 g/mol | 18.015 g/mol | 70.9 g/mol | 159.81 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | -86.8 °C | | 0 °C | -101 °C | -7.2 °C boiling point | -66.38 °C | | 99.9839 °C | -34 °C | 58.8 °C density | 0.003307 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 3.119 g/cm^3 solubility in water | miscible | | | | insoluble surface tension | 0.0271 N/m | | 0.0728 N/m | | 0.0409 N/m dynamic viscosity | 8.4×10^-4 Pa s (at -75 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 9.44×10^-4 Pa s (at 25 °C) odor | | | odorless | |

Units

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