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H2O + Cl2 + Na2S2O3 = HCl + S + Na2SO4

Input interpretation

H_2O water + Cl_2 chlorine + Na_2S_2O_3 sodium hyposulfite ⟶ HCl hydrogen chloride + S mixed sulfur + Na_2SO_4 sodium sulfate
H_2O water + Cl_2 chlorine + Na_2S_2O_3 sodium hyposulfite ⟶ HCl hydrogen chloride + S mixed sulfur + Na_2SO_4 sodium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Na_2S_2O_3 ⟶ c_4 HCl + c_5 S + c_6 Na_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Na and S: H: | 2 c_1 = c_4 O: | c_1 + 3 c_3 = 4 c_6 Cl: | 2 c_2 = c_4 Na: | 2 c_3 = 2 c_6 S: | 2 c_3 = c_5 + c_6 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 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4
Balance the chemical equation algebraically: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Na_2S_2O_3 ⟶ c_4 HCl + c_5 S + c_6 Na_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Na and S: H: | 2 c_1 = c_4 O: | c_1 + 3 c_3 = 4 c_6 Cl: | 2 c_2 = c_4 Na: | 2 c_3 = 2 c_6 S: | 2 c_3 = c_5 + c_6 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 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + chlorine + sodium hyposulfite ⟶ hydrogen chloride + mixed sulfur + sodium sulfate
water + chlorine + sodium hyposulfite ⟶ hydrogen chloride + mixed sulfur + sodium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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: H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 H_2O | 1 | -1 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) Cl_2 | 1 | -1 | ([Cl2])^(-1) Na_2S_2O_3 | 1 | -1 | ([Na2S2O3])^(-1) HCl | 2 | 2 | ([HCl])^2 S | 1 | 1 | [S] Na_2SO_4 | 1 | 1 | [Na2SO4] 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 = ([H2O])^(-1) ([Cl2])^(-1) ([Na2S2O3])^(-1) ([HCl])^2 [S] [Na2SO4] = (([HCl])^2 [S] [Na2SO4])/([H2O] [Cl2] [Na2S2O3])
Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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: H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 H_2O | 1 | -1 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) Cl_2 | 1 | -1 | ([Cl2])^(-1) Na_2S_2O_3 | 1 | -1 | ([Na2S2O3])^(-1) HCl | 2 | 2 | ([HCl])^2 S | 1 | 1 | [S] Na_2SO_4 | 1 | 1 | [Na2SO4] 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 = ([H2O])^(-1) ([Cl2])^(-1) ([Na2S2O3])^(-1) ([HCl])^2 [S] [Na2SO4] = (([HCl])^2 [S] [Na2SO4])/([H2O] [Cl2] [Na2S2O3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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: H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 H_2O | 1 | -1 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) Na_2S_2O_3 | 1 | -1 | -(Δ[Na2S2O3])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(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[H2O])/(Δt) = -(Δ[Cl2])/(Δt) = -(Δ[Na2S2O3])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[S])/(Δt) = (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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: H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 H_2O | 1 | -1 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) Na_2S_2O_3 | 1 | -1 | -(Δ[Na2S2O3])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(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[H2O])/(Δt) = -(Δ[Cl2])/(Δt) = -(Δ[Na2S2O3])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[S])/(Δt) = (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate formula | H_2O | Cl_2 | Na_2S_2O_3 | HCl | S | Na_2SO_4 Hill formula | H_2O | Cl_2 | Na_2O_3S_2 | ClH | S | Na_2O_4S name | water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate IUPAC name | water | molecular chlorine | | hydrogen chloride | sulfur | disodium sulfate
| water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate formula | H_2O | Cl_2 | Na_2S_2O_3 | HCl | S | Na_2SO_4 Hill formula | H_2O | Cl_2 | Na_2O_3S_2 | ClH | S | Na_2O_4S name | water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate IUPAC name | water | molecular chlorine | | hydrogen chloride | sulfur | disodium sulfate

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