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HCl + HMnO4 = H2O + Cl2 + MnCl2

Input interpretation

HCl hydrogen chloride + HMnO4 ⟶ H_2O water + Cl_2 chlorine + MnCl_2 manganese(II) chloride
HCl hydrogen chloride + HMnO4 ⟶ H_2O water + Cl_2 chlorine + MnCl_2 manganese(II) chloride

Balanced equation

Balance the chemical equation algebraically: HCl + HMnO4 ⟶ H_2O + Cl_2 + MnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HMnO4 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 MnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Mn and O: Cl: | c_1 = 2 c_4 + 2 c_5 H: | c_1 + c_2 = 2 c_3 Mn: | c_2 = c_5 O: | 4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 7 c_2 = 1 c_3 = 4 c_4 = 5/2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 14 c_2 = 2 c_3 = 8 c_4 = 5 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 HCl + 2 HMnO4 ⟶ 8 H_2O + 5 Cl_2 + 2 MnCl_2
Balance the chemical equation algebraically: HCl + HMnO4 ⟶ H_2O + Cl_2 + MnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HMnO4 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 MnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Mn and O: Cl: | c_1 = 2 c_4 + 2 c_5 H: | c_1 + c_2 = 2 c_3 Mn: | c_2 = c_5 O: | 4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 7 c_2 = 1 c_3 = 4 c_4 = 5/2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 14 c_2 = 2 c_3 = 8 c_4 = 5 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 14 HCl + 2 HMnO4 ⟶ 8 H_2O + 5 Cl_2 + 2 MnCl_2

Structures

+ HMnO4 ⟶ + +
+ HMnO4 ⟶ + +

Names

hydrogen chloride + HMnO4 ⟶ water + chlorine + manganese(II) chloride
hydrogen chloride + HMnO4 ⟶ water + chlorine + manganese(II) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HMnO4 ⟶ H_2O + Cl_2 + MnCl_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: 14 HCl + 2 HMnO4 ⟶ 8 H_2O + 5 Cl_2 + 2 MnCl_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 | 14 | -14 HMnO4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 MnCl_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 14 | -14 | ([HCl])^(-14) HMnO4 | 2 | -2 | ([HMnO4])^(-2) H_2O | 8 | 8 | ([H2O])^8 Cl_2 | 5 | 5 | ([Cl2])^5 MnCl_2 | 2 | 2 | ([MnCl2])^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 = ([HCl])^(-14) ([HMnO4])^(-2) ([H2O])^8 ([Cl2])^5 ([MnCl2])^2 = (([H2O])^8 ([Cl2])^5 ([MnCl2])^2)/(([HCl])^14 ([HMnO4])^2)
Construct the equilibrium constant, K, expression for: HCl + HMnO4 ⟶ H_2O + Cl_2 + MnCl_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: 14 HCl + 2 HMnO4 ⟶ 8 H_2O + 5 Cl_2 + 2 MnCl_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 | 14 | -14 HMnO4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 MnCl_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 14 | -14 | ([HCl])^(-14) HMnO4 | 2 | -2 | ([HMnO4])^(-2) H_2O | 8 | 8 | ([H2O])^8 Cl_2 | 5 | 5 | ([Cl2])^5 MnCl_2 | 2 | 2 | ([MnCl2])^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 = ([HCl])^(-14) ([HMnO4])^(-2) ([H2O])^8 ([Cl2])^5 ([MnCl2])^2 = (([H2O])^8 ([Cl2])^5 ([MnCl2])^2)/(([HCl])^14 ([HMnO4])^2)

Rate of reaction

Construct the rate of reaction expression for: HCl + HMnO4 ⟶ H_2O + Cl_2 + MnCl_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: 14 HCl + 2 HMnO4 ⟶ 8 H_2O + 5 Cl_2 + 2 MnCl_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 | 14 | -14 HMnO4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 MnCl_2 | 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 HCl | 14 | -14 | -1/14 (Δ[HCl])/(Δt) HMnO4 | 2 | -2 | -1/2 (Δ[HMnO4])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) Cl_2 | 5 | 5 | 1/5 (Δ[Cl2])/(Δt) MnCl_2 | 2 | 2 | 1/2 (Δ[MnCl2])/(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 = -1/14 (Δ[HCl])/(Δt) = -1/2 (Δ[HMnO4])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/5 (Δ[Cl2])/(Δt) = 1/2 (Δ[MnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HMnO4 ⟶ H_2O + Cl_2 + MnCl_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: 14 HCl + 2 HMnO4 ⟶ 8 H_2O + 5 Cl_2 + 2 MnCl_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 | 14 | -14 HMnO4 | 2 | -2 H_2O | 8 | 8 Cl_2 | 5 | 5 MnCl_2 | 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 HCl | 14 | -14 | -1/14 (Δ[HCl])/(Δt) HMnO4 | 2 | -2 | -1/2 (Δ[HMnO4])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) Cl_2 | 5 | 5 | 1/5 (Δ[Cl2])/(Δt) MnCl_2 | 2 | 2 | 1/2 (Δ[MnCl2])/(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 = -1/14 (Δ[HCl])/(Δt) = -1/2 (Δ[HMnO4])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/5 (Δ[Cl2])/(Δt) = 1/2 (Δ[MnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | HMnO4 | water | chlorine | manganese(II) chloride formula | HCl | HMnO4 | H_2O | Cl_2 | MnCl_2 Hill formula | ClH | HMnO4 | H_2O | Cl_2 | Cl_2Mn name | hydrogen chloride | | water | chlorine | manganese(II) chloride IUPAC name | hydrogen chloride | | water | molecular chlorine | dichloromanganese
| hydrogen chloride | HMnO4 | water | chlorine | manganese(II) chloride formula | HCl | HMnO4 | H_2O | Cl_2 | MnCl_2 Hill formula | ClH | HMnO4 | H_2O | Cl_2 | Cl_2Mn name | hydrogen chloride | | water | chlorine | manganese(II) chloride IUPAC name | hydrogen chloride | | water | molecular chlorine | dichloromanganese

Substance properties

| hydrogen chloride | HMnO4 | water | chlorine | manganese(II) chloride molar mass | 36.46 g/mol | 119.94 g/mol | 18.015 g/mol | 70.9 g/mol | 125.8 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -101 °C | 652 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 2.98 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 | HMnO4 | water | chlorine | manganese(II) chloride molar mass | 36.46 g/mol | 119.94 g/mol | 18.015 g/mol | 70.9 g/mol | 125.8 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -101 °C | 652 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 2.98 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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