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NaCl + HClO = H2O + Cl2 + NaClO

Input interpretation

NaCl sodium chloride + HOCl hypochlorous acid ⟶ H_2O water + Cl_2 chlorine + NaOCl sodium hypochlorite
NaCl sodium chloride + HOCl hypochlorous acid ⟶ H_2O water + Cl_2 chlorine + NaOCl sodium hypochlorite

Balanced equation

Balance the chemical equation algebraically: NaCl + HOCl ⟶ H_2O + Cl_2 + NaOCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaCl + c_2 HOCl ⟶ c_3 H_2O + c_4 Cl_2 + c_5 NaOCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na, H and O: Cl: | c_1 + c_2 = 2 c_4 + c_5 Na: | c_1 = c_5 H: | c_2 = 2 c_3 O: | c_2 = c_3 + c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaCl + 2 HOCl ⟶ H_2O + Cl_2 + NaOCl
Balance the chemical equation algebraically: NaCl + HOCl ⟶ H_2O + Cl_2 + NaOCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaCl + c_2 HOCl ⟶ c_3 H_2O + c_4 Cl_2 + c_5 NaOCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na, H and O: Cl: | c_1 + c_2 = 2 c_4 + c_5 Na: | c_1 = c_5 H: | c_2 = 2 c_3 O: | c_2 = c_3 + c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaCl + 2 HOCl ⟶ H_2O + Cl_2 + NaOCl

Structures

+ ⟶ + +
+ ⟶ + +

Names

sodium chloride + hypochlorous acid ⟶ water + chlorine + sodium hypochlorite
sodium chloride + hypochlorous acid ⟶ water + chlorine + sodium hypochlorite

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaCl + HOCl ⟶ H_2O + Cl_2 + NaOCl 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: NaCl + 2 HOCl ⟶ H_2O + Cl_2 + NaOCl 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 NaCl | 1 | -1 HOCl | 2 | -2 H_2O | 1 | 1 Cl_2 | 1 | 1 NaOCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaCl | 1 | -1 | ([NaCl])^(-1) HOCl | 2 | -2 | ([HOCl])^(-2) H_2O | 1 | 1 | [H2O] Cl_2 | 1 | 1 | [Cl2] NaOCl | 1 | 1 | [NaOCl] 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 = ([NaCl])^(-1) ([HOCl])^(-2) [H2O] [Cl2] [NaOCl] = ([H2O] [Cl2] [NaOCl])/([NaCl] ([HOCl])^2)
Construct the equilibrium constant, K, expression for: NaCl + HOCl ⟶ H_2O + Cl_2 + NaOCl 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: NaCl + 2 HOCl ⟶ H_2O + Cl_2 + NaOCl 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 NaCl | 1 | -1 HOCl | 2 | -2 H_2O | 1 | 1 Cl_2 | 1 | 1 NaOCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaCl | 1 | -1 | ([NaCl])^(-1) HOCl | 2 | -2 | ([HOCl])^(-2) H_2O | 1 | 1 | [H2O] Cl_2 | 1 | 1 | [Cl2] NaOCl | 1 | 1 | [NaOCl] 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 = ([NaCl])^(-1) ([HOCl])^(-2) [H2O] [Cl2] [NaOCl] = ([H2O] [Cl2] [NaOCl])/([NaCl] ([HOCl])^2)

Rate of reaction

Construct the rate of reaction expression for: NaCl + HOCl ⟶ H_2O + Cl_2 + NaOCl 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: NaCl + 2 HOCl ⟶ H_2O + Cl_2 + NaOCl 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 NaCl | 1 | -1 HOCl | 2 | -2 H_2O | 1 | 1 Cl_2 | 1 | 1 NaOCl | 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 NaCl | 1 | -1 | -(Δ[NaCl])/(Δt) HOCl | 2 | -2 | -1/2 (Δ[HOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) NaOCl | 1 | 1 | (Δ[NaOCl])/(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 = -(Δ[NaCl])/(Δt) = -1/2 (Δ[HOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = (Δ[NaOCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaCl + HOCl ⟶ H_2O + Cl_2 + NaOCl 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: NaCl + 2 HOCl ⟶ H_2O + Cl_2 + NaOCl 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 NaCl | 1 | -1 HOCl | 2 | -2 H_2O | 1 | 1 Cl_2 | 1 | 1 NaOCl | 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 NaCl | 1 | -1 | -(Δ[NaCl])/(Δt) HOCl | 2 | -2 | -1/2 (Δ[HOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) NaOCl | 1 | 1 | (Δ[NaOCl])/(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 = -(Δ[NaCl])/(Δt) = -1/2 (Δ[HOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = (Δ[NaOCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium chloride | hypochlorous acid | water | chlorine | sodium hypochlorite formula | NaCl | HOCl | H_2O | Cl_2 | NaOCl Hill formula | ClNa | ClHO | H_2O | Cl_2 | ClNaO name | sodium chloride | hypochlorous acid | water | chlorine | sodium hypochlorite IUPAC name | sodium chloride | hypochlorous acid | water | molecular chlorine | sodium hypochlorite
| sodium chloride | hypochlorous acid | water | chlorine | sodium hypochlorite formula | NaCl | HOCl | H_2O | Cl_2 | NaOCl Hill formula | ClNa | ClHO | H_2O | Cl_2 | ClNaO name | sodium chloride | hypochlorous acid | water | chlorine | sodium hypochlorite IUPAC name | sodium chloride | hypochlorous acid | water | molecular chlorine | sodium hypochlorite

Substance properties

| sodium chloride | hypochlorous acid | water | chlorine | sodium hypochlorite molar mass | 58.44 g/mol | 52.46 g/mol | 18.015 g/mol | 70.9 g/mol | 74.44 g/mol phase | solid (at STP) | | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | 801 °C | | 0 °C | -101 °C | -6 °C boiling point | 1413 °C | | 99.9839 °C | -34 °C | density | 2.16 g/cm^3 | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 1.11 g/cm^3 solubility in water | soluble | soluble | | | miscible surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |
| sodium chloride | hypochlorous acid | water | chlorine | sodium hypochlorite molar mass | 58.44 g/mol | 52.46 g/mol | 18.015 g/mol | 70.9 g/mol | 74.44 g/mol phase | solid (at STP) | | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | 801 °C | | 0 °C | -101 °C | -6 °C boiling point | 1413 °C | | 99.9839 °C | -34 °C | density | 2.16 g/cm^3 | | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 1.11 g/cm^3 solubility in water | soluble | soluble | | | miscible surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |

Units

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