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HCl + FeCl2 + HClO3 = H2O + FeCl3

Input interpretation

HCl hydrogen chloride + FeCl_2 iron(II) chloride + HClO3 ⟶ H_2O water + FeCl_3 iron(III) chloride
HCl hydrogen chloride + FeCl_2 iron(II) chloride + HClO3 ⟶ H_2O water + FeCl_3 iron(III) chloride

Balanced equation

Balance the chemical equation algebraically: HCl + FeCl_2 + HClO3 ⟶ H_2O + FeCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 FeCl_2 + c_3 HClO3 ⟶ c_4 H_2O + c_5 FeCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Fe and O: Cl: | c_1 + 2 c_2 + c_3 = 3 c_5 H: | c_1 + c_3 = 2 c_4 Fe: | c_2 = 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 = 5 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 HCl + 6 FeCl_2 + HClO3 ⟶ 3 H_2O + 6 FeCl_3
Balance the chemical equation algebraically: HCl + FeCl_2 + HClO3 ⟶ H_2O + FeCl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 FeCl_2 + c_3 HClO3 ⟶ c_4 H_2O + c_5 FeCl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Fe and O: Cl: | c_1 + 2 c_2 + c_3 = 3 c_5 H: | c_1 + c_3 = 2 c_4 Fe: | c_2 = 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 = 5 c_2 = 6 c_3 = 1 c_4 = 3 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 HCl + 6 FeCl_2 + HClO3 ⟶ 3 H_2O + 6 FeCl_3

Structures

+ + HClO3 ⟶ +
+ + HClO3 ⟶ +

Names

hydrogen chloride + iron(II) chloride + HClO3 ⟶ water + iron(III) chloride
hydrogen chloride + iron(II) chloride + HClO3 ⟶ water + iron(III) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + FeCl_2 + HClO3 ⟶ H_2O + FeCl_3 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: 5 HCl + 6 FeCl_2 + HClO3 ⟶ 3 H_2O + 6 FeCl_3 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 | 5 | -5 FeCl_2 | 6 | -6 HClO3 | 1 | -1 H_2O | 3 | 3 FeCl_3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 5 | -5 | ([HCl])^(-5) FeCl_2 | 6 | -6 | ([FeCl2])^(-6) HClO3 | 1 | -1 | ([HClO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 FeCl_3 | 6 | 6 | ([FeCl3])^6 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])^(-5) ([FeCl2])^(-6) ([HClO3])^(-1) ([H2O])^3 ([FeCl3])^6 = (([H2O])^3 ([FeCl3])^6)/(([HCl])^5 ([FeCl2])^6 [HClO3])
Construct the equilibrium constant, K, expression for: HCl + FeCl_2 + HClO3 ⟶ H_2O + FeCl_3 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: 5 HCl + 6 FeCl_2 + HClO3 ⟶ 3 H_2O + 6 FeCl_3 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 | 5 | -5 FeCl_2 | 6 | -6 HClO3 | 1 | -1 H_2O | 3 | 3 FeCl_3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 5 | -5 | ([HCl])^(-5) FeCl_2 | 6 | -6 | ([FeCl2])^(-6) HClO3 | 1 | -1 | ([HClO3])^(-1) H_2O | 3 | 3 | ([H2O])^3 FeCl_3 | 6 | 6 | ([FeCl3])^6 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])^(-5) ([FeCl2])^(-6) ([HClO3])^(-1) ([H2O])^3 ([FeCl3])^6 = (([H2O])^3 ([FeCl3])^6)/(([HCl])^5 ([FeCl2])^6 [HClO3])

Rate of reaction

Construct the rate of reaction expression for: HCl + FeCl_2 + HClO3 ⟶ H_2O + FeCl_3 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: 5 HCl + 6 FeCl_2 + HClO3 ⟶ 3 H_2O + 6 FeCl_3 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 | 5 | -5 FeCl_2 | 6 | -6 HClO3 | 1 | -1 H_2O | 3 | 3 FeCl_3 | 6 | 6 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 | 5 | -5 | -1/5 (Δ[HCl])/(Δt) FeCl_2 | 6 | -6 | -1/6 (Δ[FeCl2])/(Δt) HClO3 | 1 | -1 | -(Δ[HClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) FeCl_3 | 6 | 6 | 1/6 (Δ[FeCl3])/(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 = -1/5 (Δ[HCl])/(Δt) = -1/6 (Δ[FeCl2])/(Δt) = -(Δ[HClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/6 (Δ[FeCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + FeCl_2 + HClO3 ⟶ H_2O + FeCl_3 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: 5 HCl + 6 FeCl_2 + HClO3 ⟶ 3 H_2O + 6 FeCl_3 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 | 5 | -5 FeCl_2 | 6 | -6 HClO3 | 1 | -1 H_2O | 3 | 3 FeCl_3 | 6 | 6 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 | 5 | -5 | -1/5 (Δ[HCl])/(Δt) FeCl_2 | 6 | -6 | -1/6 (Δ[FeCl2])/(Δt) HClO3 | 1 | -1 | -(Δ[HClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) FeCl_3 | 6 | 6 | 1/6 (Δ[FeCl3])/(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 = -1/5 (Δ[HCl])/(Δt) = -1/6 (Δ[FeCl2])/(Δt) = -(Δ[HClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/6 (Δ[FeCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | iron(II) chloride | HClO3 | water | iron(III) chloride formula | HCl | FeCl_2 | HClO3 | H_2O | FeCl_3 Hill formula | ClH | Cl_2Fe | HClO3 | H_2O | Cl_3Fe name | hydrogen chloride | iron(II) chloride | | water | iron(III) chloride IUPAC name | hydrogen chloride | dichloroiron | | water | trichloroiron
| hydrogen chloride | iron(II) chloride | HClO3 | water | iron(III) chloride formula | HCl | FeCl_2 | HClO3 | H_2O | FeCl_3 Hill formula | ClH | Cl_2Fe | HClO3 | H_2O | Cl_3Fe name | hydrogen chloride | iron(II) chloride | | water | iron(III) chloride IUPAC name | hydrogen chloride | dichloroiron | | water | trichloroiron

Substance properties

| hydrogen chloride | iron(II) chloride | HClO3 | water | iron(III) chloride molar mass | 36.46 g/mol | 126.7 g/mol | 84.45 g/mol | 18.015 g/mol | 162.2 g/mol phase | gas (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 677 °C | | 0 °C | 304 °C boiling point | -85 °C | | | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | 3.16 g/cm^3 | | 1 g/cm^3 | solubility in water | miscible | | | | surface tension | | | | 0.0728 N/m | dynamic viscosity | | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | | odorless |
| hydrogen chloride | iron(II) chloride | HClO3 | water | iron(III) chloride molar mass | 36.46 g/mol | 126.7 g/mol | 84.45 g/mol | 18.015 g/mol | 162.2 g/mol phase | gas (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 677 °C | | 0 °C | 304 °C boiling point | -85 °C | | | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | 3.16 g/cm^3 | | 1 g/cm^3 | solubility in water | miscible | | | | surface tension | | | | 0.0728 N/m | dynamic viscosity | | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | | odorless |

Units

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