Input interpretation
![HCl hydrogen chloride + KClO2 ⟶ H_2O water + Cl_2 chlorine + KCl potassium chloride](../image_source/96b91b7ec5eed6b9d846de1a95696684.png)
HCl hydrogen chloride + KClO2 ⟶ H_2O water + Cl_2 chlorine + KCl potassium chloride
Balanced equation
![Balance the chemical equation algebraically: HCl + KClO2 ⟶ H_2O + Cl_2 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KClO2 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K and O: Cl: | c_1 + c_2 = 2 c_4 + c_5 H: | c_1 = 2 c_3 K: | c_2 = c_5 O: | 2 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 = 4 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + KClO2 ⟶ 2 H_2O + 2 Cl_2 + KCl](../image_source/d166b1ba933b4f9f308149960aecd588.png)
Balance the chemical equation algebraically: HCl + KClO2 ⟶ H_2O + Cl_2 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KClO2 ⟶ c_3 H_2O + c_4 Cl_2 + c_5 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K and O: Cl: | c_1 + c_2 = 2 c_4 + c_5 H: | c_1 = 2 c_3 K: | c_2 = c_5 O: | 2 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 = 4 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + KClO2 ⟶ 2 H_2O + 2 Cl_2 + KCl
Structures
![+ KClO2 ⟶ + +](../image_source/d3e9d67d188f308b6893a7984ae979bc.png)
+ KClO2 ⟶ + +
Names
![hydrogen chloride + KClO2 ⟶ water + chlorine + potassium chloride](../image_source/2f09eef5b25e541f6cd2bdcbb12c5002.png)
hydrogen chloride + KClO2 ⟶ water + chlorine + potassium chloride
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + KClO2 ⟶ H_2O + Cl_2 + KCl 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: 4 HCl + KClO2 ⟶ 2 H_2O + 2 Cl_2 + KCl 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 | 4 | -4 KClO2 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 KCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) KClO2 | 1 | -1 | ([KClO2])^(-1) H_2O | 2 | 2 | ([H2O])^2 Cl_2 | 2 | 2 | ([Cl2])^2 KCl | 1 | 1 | [KCl] 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])^(-4) ([KClO2])^(-1) ([H2O])^2 ([Cl2])^2 [KCl] = (([H2O])^2 ([Cl2])^2 [KCl])/(([HCl])^4 [KClO2])](../image_source/e0b75c77df878dc9de8a29e2403403cf.png)
Construct the equilibrium constant, K, expression for: HCl + KClO2 ⟶ H_2O + Cl_2 + KCl 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: 4 HCl + KClO2 ⟶ 2 H_2O + 2 Cl_2 + KCl 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 | 4 | -4 KClO2 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 KCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) KClO2 | 1 | -1 | ([KClO2])^(-1) H_2O | 2 | 2 | ([H2O])^2 Cl_2 | 2 | 2 | ([Cl2])^2 KCl | 1 | 1 | [KCl] 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])^(-4) ([KClO2])^(-1) ([H2O])^2 ([Cl2])^2 [KCl] = (([H2O])^2 ([Cl2])^2 [KCl])/(([HCl])^4 [KClO2])
Rate of reaction
![Construct the rate of reaction expression for: HCl + KClO2 ⟶ H_2O + Cl_2 + KCl 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: 4 HCl + KClO2 ⟶ 2 H_2O + 2 Cl_2 + KCl 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 | 4 | -4 KClO2 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 KCl | 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 HCl | 4 | -4 | -1/4 (Δ[HCl])/(Δt) KClO2 | 1 | -1 | -(Δ[KClO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Cl_2 | 2 | 2 | 1/2 (Δ[Cl2])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(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 = -1/4 (Δ[HCl])/(Δt) = -(Δ[KClO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[Cl2])/(Δt) = (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/54f552238b511b22f3ea7d82a2467ce8.png)
Construct the rate of reaction expression for: HCl + KClO2 ⟶ H_2O + Cl_2 + KCl 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: 4 HCl + KClO2 ⟶ 2 H_2O + 2 Cl_2 + KCl 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 | 4 | -4 KClO2 | 1 | -1 H_2O | 2 | 2 Cl_2 | 2 | 2 KCl | 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 HCl | 4 | -4 | -1/4 (Δ[HCl])/(Δt) KClO2 | 1 | -1 | -(Δ[KClO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Cl_2 | 2 | 2 | 1/2 (Δ[Cl2])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(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 = -1/4 (Δ[HCl])/(Δt) = -(Δ[KClO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[Cl2])/(Δt) = (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen chloride | KClO2 | water | chlorine | potassium chloride formula | HCl | KClO2 | H_2O | Cl_2 | KCl Hill formula | ClH | ClKO2 | H_2O | Cl_2 | ClK name | hydrogen chloride | | water | chlorine | potassium chloride IUPAC name | hydrogen chloride | | water | molecular chlorine | potassium chloride](../image_source/2bd2d6fc4393c931df99a9be062704d9.png)
| hydrogen chloride | KClO2 | water | chlorine | potassium chloride formula | HCl | KClO2 | H_2O | Cl_2 | KCl Hill formula | ClH | ClKO2 | H_2O | Cl_2 | ClK name | hydrogen chloride | | water | chlorine | potassium chloride IUPAC name | hydrogen chloride | | water | molecular chlorine | potassium chloride
Substance properties
![| hydrogen chloride | KClO2 | water | chlorine | potassium chloride molar mass | 36.46 g/mol | 106.5 g/mol | 18.015 g/mol | 70.9 g/mol | 74.55 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -101 °C | 770 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | 1420 °C density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 1.98 g/cm^3 solubility in water | miscible | | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | | odorless](../image_source/ff17807266d4aaecd8e6de0385c5c008.png)
| hydrogen chloride | KClO2 | water | chlorine | potassium chloride molar mass | 36.46 g/mol | 106.5 g/mol | 18.015 g/mol | 70.9 g/mol | 74.55 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -101 °C | 770 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | 1420 °C density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 1.98 g/cm^3 solubility in water | miscible | | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | | odorless
Units