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H2O + Cl2 + As2S3 = H2SO4 + HCl + H3AsO4

Input interpretation

H_2O water + Cl_2 chlorine + As_2S_3 arsenic(III) sulfide ⟶ H_2SO_4 sulfuric acid + HCl hydrogen chloride + H_3AsO_4 arsenic acid, solid
H_2O water + Cl_2 chlorine + As_2S_3 arsenic(III) sulfide ⟶ H_2SO_4 sulfuric acid + HCl hydrogen chloride + H_3AsO_4 arsenic acid, solid

Balanced equation

Balance the chemical equation algebraically: H_2O + Cl_2 + As_2S_3 ⟶ H_2SO_4 + HCl + H_3AsO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 As_2S_3 ⟶ c_4 H_2SO_4 + c_5 HCl + c_6 H_3AsO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, As and S: H: | 2 c_1 = 2 c_4 + c_5 + 3 c_6 O: | c_1 = 4 c_4 + 4 c_6 Cl: | 2 c_2 = c_5 As: | 2 c_3 = c_6 S: | 3 c_3 = c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 20 c_2 = 14 c_3 = 1 c_4 = 3 c_5 = 28 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 20 H_2O + 14 Cl_2 + As_2S_3 ⟶ 3 H_2SO_4 + 28 HCl + 2 H_3AsO_4
Balance the chemical equation algebraically: H_2O + Cl_2 + As_2S_3 ⟶ H_2SO_4 + HCl + H_3AsO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 As_2S_3 ⟶ c_4 H_2SO_4 + c_5 HCl + c_6 H_3AsO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, As and S: H: | 2 c_1 = 2 c_4 + c_5 + 3 c_6 O: | c_1 = 4 c_4 + 4 c_6 Cl: | 2 c_2 = c_5 As: | 2 c_3 = c_6 S: | 3 c_3 = c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 20 c_2 = 14 c_3 = 1 c_4 = 3 c_5 = 28 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 20 H_2O + 14 Cl_2 + As_2S_3 ⟶ 3 H_2SO_4 + 28 HCl + 2 H_3AsO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + chlorine + arsenic(III) sulfide ⟶ sulfuric acid + hydrogen chloride + arsenic acid, solid
water + chlorine + arsenic(III) sulfide ⟶ sulfuric acid + hydrogen chloride + arsenic acid, solid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + As_2S_3 ⟶ H_2SO_4 + HCl + H_3AsO_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: 20 H_2O + 14 Cl_2 + As_2S_3 ⟶ 3 H_2SO_4 + 28 HCl + 2 H_3AsO_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 | 20 | -20 Cl_2 | 14 | -14 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 HCl | 28 | 28 H_3AsO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 20 | -20 | ([H2O])^(-20) Cl_2 | 14 | -14 | ([Cl2])^(-14) As_2S_3 | 1 | -1 | ([As2S3])^(-1) H_2SO_4 | 3 | 3 | ([H2SO4])^3 HCl | 28 | 28 | ([HCl])^28 H_3AsO_4 | 2 | 2 | ([H3AsO4])^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 = ([H2O])^(-20) ([Cl2])^(-14) ([As2S3])^(-1) ([H2SO4])^3 ([HCl])^28 ([H3AsO4])^2 = (([H2SO4])^3 ([HCl])^28 ([H3AsO4])^2)/(([H2O])^20 ([Cl2])^14 [As2S3])
Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + As_2S_3 ⟶ H_2SO_4 + HCl + H_3AsO_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: 20 H_2O + 14 Cl_2 + As_2S_3 ⟶ 3 H_2SO_4 + 28 HCl + 2 H_3AsO_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 | 20 | -20 Cl_2 | 14 | -14 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 HCl | 28 | 28 H_3AsO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 20 | -20 | ([H2O])^(-20) Cl_2 | 14 | -14 | ([Cl2])^(-14) As_2S_3 | 1 | -1 | ([As2S3])^(-1) H_2SO_4 | 3 | 3 | ([H2SO4])^3 HCl | 28 | 28 | ([HCl])^28 H_3AsO_4 | 2 | 2 | ([H3AsO4])^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 = ([H2O])^(-20) ([Cl2])^(-14) ([As2S3])^(-1) ([H2SO4])^3 ([HCl])^28 ([H3AsO4])^2 = (([H2SO4])^3 ([HCl])^28 ([H3AsO4])^2)/(([H2O])^20 ([Cl2])^14 [As2S3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + Cl_2 + As_2S_3 ⟶ H_2SO_4 + HCl + H_3AsO_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: 20 H_2O + 14 Cl_2 + As_2S_3 ⟶ 3 H_2SO_4 + 28 HCl + 2 H_3AsO_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 | 20 | -20 Cl_2 | 14 | -14 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 HCl | 28 | 28 H_3AsO_4 | 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 H_2O | 20 | -20 | -1/20 (Δ[H2O])/(Δt) Cl_2 | 14 | -14 | -1/14 (Δ[Cl2])/(Δt) As_2S_3 | 1 | -1 | -(Δ[As2S3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) HCl | 28 | 28 | 1/28 (Δ[HCl])/(Δt) H_3AsO_4 | 2 | 2 | 1/2 (Δ[H3AsO4])/(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 = -1/20 (Δ[H2O])/(Δt) = -1/14 (Δ[Cl2])/(Δt) = -(Δ[As2S3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/28 (Δ[HCl])/(Δt) = 1/2 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Cl_2 + As_2S_3 ⟶ H_2SO_4 + HCl + H_3AsO_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: 20 H_2O + 14 Cl_2 + As_2S_3 ⟶ 3 H_2SO_4 + 28 HCl + 2 H_3AsO_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 | 20 | -20 Cl_2 | 14 | -14 As_2S_3 | 1 | -1 H_2SO_4 | 3 | 3 HCl | 28 | 28 H_3AsO_4 | 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 H_2O | 20 | -20 | -1/20 (Δ[H2O])/(Δt) Cl_2 | 14 | -14 | -1/14 (Δ[Cl2])/(Δt) As_2S_3 | 1 | -1 | -(Δ[As2S3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) HCl | 28 | 28 | 1/28 (Δ[HCl])/(Δt) H_3AsO_4 | 2 | 2 | 1/2 (Δ[H3AsO4])/(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 = -1/20 (Δ[H2O])/(Δt) = -1/14 (Δ[Cl2])/(Δt) = -(Δ[As2S3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/28 (Δ[HCl])/(Δt) = 1/2 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | chlorine | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid formula | H_2O | Cl_2 | As_2S_3 | H_2SO_4 | HCl | H_3AsO_4 Hill formula | H_2O | Cl_2 | As_2S_3 | H_2O_4S | ClH | AsH_3O_4 name | water | chlorine | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid IUPAC name | water | molecular chlorine | | sulfuric acid | hydrogen chloride | arsoric acid
| water | chlorine | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid formula | H_2O | Cl_2 | As_2S_3 | H_2SO_4 | HCl | H_3AsO_4 Hill formula | H_2O | Cl_2 | As_2S_3 | H_2O_4S | ClH | AsH_3O_4 name | water | chlorine | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid IUPAC name | water | molecular chlorine | | sulfuric acid | hydrogen chloride | arsoric acid

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