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Cl2 + NaOH = H2O + Na + NaClO3

Input interpretation

Cl_2 chlorine + NaOH sodium hydroxide ⟶ H_2O water + Na sodium + NaClO_3 sodium chlorate
Cl_2 chlorine + NaOH sodium hydroxide ⟶ H_2O water + Na sodium + NaClO_3 sodium chlorate

Balanced equation

Balance the chemical equation algebraically: Cl_2 + NaOH ⟶ H_2O + Na + NaClO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 NaOH ⟶ c_3 H_2O + c_4 Na + c_5 NaClO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na and O: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_3 Na: | c_2 = c_4 + c_5 O: | c_2 = c_3 + 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 = 12 c_3 = 6 c_4 = 10 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 12 NaOH ⟶ 6 H_2O + 10 Na + 2 NaClO_3
Balance the chemical equation algebraically: Cl_2 + NaOH ⟶ H_2O + Na + NaClO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 NaOH ⟶ c_3 H_2O + c_4 Na + c_5 NaClO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na and O: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_3 Na: | c_2 = c_4 + c_5 O: | c_2 = c_3 + 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 = 12 c_3 = 6 c_4 = 10 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 12 NaOH ⟶ 6 H_2O + 10 Na + 2 NaClO_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

chlorine + sodium hydroxide ⟶ water + sodium + sodium chlorate
chlorine + sodium hydroxide ⟶ water + sodium + sodium chlorate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + NaOH ⟶ H_2O + Na + NaClO_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: Cl_2 + 12 NaOH ⟶ 6 H_2O + 10 Na + 2 NaClO_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 Cl_2 | 1 | -1 NaOH | 12 | -12 H_2O | 6 | 6 Na | 10 | 10 NaClO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) NaOH | 12 | -12 | ([NaOH])^(-12) H_2O | 6 | 6 | ([H2O])^6 Na | 10 | 10 | ([Na])^10 NaClO_3 | 2 | 2 | ([NaClO3])^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 = ([Cl2])^(-1) ([NaOH])^(-12) ([H2O])^6 ([Na])^10 ([NaClO3])^2 = (([H2O])^6 ([Na])^10 ([NaClO3])^2)/([Cl2] ([NaOH])^12)
Construct the equilibrium constant, K, expression for: Cl_2 + NaOH ⟶ H_2O + Na + NaClO_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: Cl_2 + 12 NaOH ⟶ 6 H_2O + 10 Na + 2 NaClO_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 Cl_2 | 1 | -1 NaOH | 12 | -12 H_2O | 6 | 6 Na | 10 | 10 NaClO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) NaOH | 12 | -12 | ([NaOH])^(-12) H_2O | 6 | 6 | ([H2O])^6 Na | 10 | 10 | ([Na])^10 NaClO_3 | 2 | 2 | ([NaClO3])^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 = ([Cl2])^(-1) ([NaOH])^(-12) ([H2O])^6 ([Na])^10 ([NaClO3])^2 = (([H2O])^6 ([Na])^10 ([NaClO3])^2)/([Cl2] ([NaOH])^12)

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + NaOH ⟶ H_2O + Na + NaClO_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: Cl_2 + 12 NaOH ⟶ 6 H_2O + 10 Na + 2 NaClO_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 Cl_2 | 1 | -1 NaOH | 12 | -12 H_2O | 6 | 6 Na | 10 | 10 NaClO_3 | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) NaOH | 12 | -12 | -1/12 (Δ[NaOH])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) Na | 10 | 10 | 1/10 (Δ[Na])/(Δt) NaClO_3 | 2 | 2 | 1/2 (Δ[NaClO3])/(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[Cl2])/(Δt) = -1/12 (Δ[NaOH])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/10 (Δ[Na])/(Δt) = 1/2 (Δ[NaClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + NaOH ⟶ H_2O + Na + NaClO_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: Cl_2 + 12 NaOH ⟶ 6 H_2O + 10 Na + 2 NaClO_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 Cl_2 | 1 | -1 NaOH | 12 | -12 H_2O | 6 | 6 Na | 10 | 10 NaClO_3 | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) NaOH | 12 | -12 | -1/12 (Δ[NaOH])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) Na | 10 | 10 | 1/10 (Δ[Na])/(Δt) NaClO_3 | 2 | 2 | 1/2 (Δ[NaClO3])/(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[Cl2])/(Δt) = -1/12 (Δ[NaOH])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/10 (Δ[Na])/(Δt) = 1/2 (Δ[NaClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | sodium hydroxide | water | sodium | sodium chlorate formula | Cl_2 | NaOH | H_2O | Na | NaClO_3 Hill formula | Cl_2 | HNaO | H_2O | Na | ClNaO_3 name | chlorine | sodium hydroxide | water | sodium | sodium chlorate IUPAC name | molecular chlorine | sodium hydroxide | water | sodium | sodium chlorate
| chlorine | sodium hydroxide | water | sodium | sodium chlorate formula | Cl_2 | NaOH | H_2O | Na | NaClO_3 Hill formula | Cl_2 | HNaO | H_2O | Na | ClNaO_3 name | chlorine | sodium hydroxide | water | sodium | sodium chlorate IUPAC name | molecular chlorine | sodium hydroxide | water | sodium | sodium chlorate

Substance properties

| chlorine | sodium hydroxide | water | sodium | sodium chlorate molar mass | 70.9 g/mol | 39.997 g/mol | 18.015 g/mol | 22.98976928 g/mol | 106.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) melting point | -101 °C | 323 °C | 0 °C | 97.8 °C | boiling point | -34 °C | 1390 °C | 99.9839 °C | 883 °C | 106 °C density | 0.003214 g/cm^3 (at 0 °C) | 2.13 g/cm^3 | 1 g/cm^3 | 0.968 g/cm^3 | 1.3 g/cm^3 solubility in water | | soluble | | decomposes | very soluble surface tension | | 0.07435 N/m | 0.0728 N/m | | dynamic viscosity | | 0.004 Pa s (at 350 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.413×10^-5 Pa s (at 527 °C) | 0.00542 Pa s (at 286 °C) odor | | | odorless | | odorless
| chlorine | sodium hydroxide | water | sodium | sodium chlorate molar mass | 70.9 g/mol | 39.997 g/mol | 18.015 g/mol | 22.98976928 g/mol | 106.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) melting point | -101 °C | 323 °C | 0 °C | 97.8 °C | boiling point | -34 °C | 1390 °C | 99.9839 °C | 883 °C | 106 °C density | 0.003214 g/cm^3 (at 0 °C) | 2.13 g/cm^3 | 1 g/cm^3 | 0.968 g/cm^3 | 1.3 g/cm^3 solubility in water | | soluble | | decomposes | very soluble surface tension | | 0.07435 N/m | 0.0728 N/m | | dynamic viscosity | | 0.004 Pa s (at 350 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.413×10^-5 Pa s (at 527 °C) | 0.00542 Pa s (at 286 °C) odor | | | odorless | | odorless

Units

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