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H2O + HClO3 + As2S3 = H2SO4 + HCl + H3AsO4

Input interpretation

H_2O water + HClO3 + As_2S_3 arsenic(III) sulfide ⟶ H_2SO_4 sulfuric acid + HCl hydrogen chloride + H_3AsO_4 arsenic acid, solid
H_2O water + HClO3 + 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 + HClO3 + 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 HClO3 + 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 + c_2 = 2 c_4 + c_5 + 3 c_6 O: | c_1 + 3 c_2 = 4 c_4 + 4 c_6 Cl: | 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 = 6 c_2 = 14/3 c_3 = 1 c_4 = 3 c_5 = 14/3 c_6 = 2 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 18 c_2 = 14 c_3 = 3 c_4 = 9 c_5 = 14 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 18 H_2O + 14 HClO3 + 3 As_2S_3 ⟶ 9 H_2SO_4 + 14 HCl + 6 H_3AsO_4
Balance the chemical equation algebraically: H_2O + HClO3 + 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 HClO3 + 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 + c_2 = 2 c_4 + c_5 + 3 c_6 O: | c_1 + 3 c_2 = 4 c_4 + 4 c_6 Cl: | 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 = 6 c_2 = 14/3 c_3 = 1 c_4 = 3 c_5 = 14/3 c_6 = 2 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 18 c_2 = 14 c_3 = 3 c_4 = 9 c_5 = 14 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 18 H_2O + 14 HClO3 + 3 As_2S_3 ⟶ 9 H_2SO_4 + 14 HCl + 6 H_3AsO_4

Structures

+ HClO3 + ⟶ + +
+ HClO3 + ⟶ + +

Names

water + HClO3 + arsenic(III) sulfide ⟶ sulfuric acid + hydrogen chloride + arsenic acid, solid
water + HClO3 + arsenic(III) sulfide ⟶ sulfuric acid + hydrogen chloride + arsenic acid, solid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HClO3 + 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: 18 H_2O + 14 HClO3 + 3 As_2S_3 ⟶ 9 H_2SO_4 + 14 HCl + 6 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 | 18 | -18 HClO3 | 14 | -14 As_2S_3 | 3 | -3 H_2SO_4 | 9 | 9 HCl | 14 | 14 H_3AsO_4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 18 | -18 | ([H2O])^(-18) HClO3 | 14 | -14 | ([HClO3])^(-14) As_2S_3 | 3 | -3 | ([As2S3])^(-3) H_2SO_4 | 9 | 9 | ([H2SO4])^9 HCl | 14 | 14 | ([HCl])^14 H_3AsO_4 | 6 | 6 | ([H3AsO4])^6 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])^(-18) ([HClO3])^(-14) ([As2S3])^(-3) ([H2SO4])^9 ([HCl])^14 ([H3AsO4])^6 = (([H2SO4])^9 ([HCl])^14 ([H3AsO4])^6)/(([H2O])^18 ([HClO3])^14 ([As2S3])^3)
Construct the equilibrium constant, K, expression for: H_2O + HClO3 + 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: 18 H_2O + 14 HClO3 + 3 As_2S_3 ⟶ 9 H_2SO_4 + 14 HCl + 6 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 | 18 | -18 HClO3 | 14 | -14 As_2S_3 | 3 | -3 H_2SO_4 | 9 | 9 HCl | 14 | 14 H_3AsO_4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 18 | -18 | ([H2O])^(-18) HClO3 | 14 | -14 | ([HClO3])^(-14) As_2S_3 | 3 | -3 | ([As2S3])^(-3) H_2SO_4 | 9 | 9 | ([H2SO4])^9 HCl | 14 | 14 | ([HCl])^14 H_3AsO_4 | 6 | 6 | ([H3AsO4])^6 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])^(-18) ([HClO3])^(-14) ([As2S3])^(-3) ([H2SO4])^9 ([HCl])^14 ([H3AsO4])^6 = (([H2SO4])^9 ([HCl])^14 ([H3AsO4])^6)/(([H2O])^18 ([HClO3])^14 ([As2S3])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2O + HClO3 + 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: 18 H_2O + 14 HClO3 + 3 As_2S_3 ⟶ 9 H_2SO_4 + 14 HCl + 6 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 | 18 | -18 HClO3 | 14 | -14 As_2S_3 | 3 | -3 H_2SO_4 | 9 | 9 HCl | 14 | 14 H_3AsO_4 | 6 | 6 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 | 18 | -18 | -1/18 (Δ[H2O])/(Δt) HClO3 | 14 | -14 | -1/14 (Δ[HClO3])/(Δt) As_2S_3 | 3 | -3 | -1/3 (Δ[As2S3])/(Δt) H_2SO_4 | 9 | 9 | 1/9 (Δ[H2SO4])/(Δt) HCl | 14 | 14 | 1/14 (Δ[HCl])/(Δt) H_3AsO_4 | 6 | 6 | 1/6 (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 = -1/18 (Δ[H2O])/(Δt) = -1/14 (Δ[HClO3])/(Δt) = -1/3 (Δ[As2S3])/(Δt) = 1/9 (Δ[H2SO4])/(Δt) = 1/14 (Δ[HCl])/(Δt) = 1/6 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HClO3 + 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: 18 H_2O + 14 HClO3 + 3 As_2S_3 ⟶ 9 H_2SO_4 + 14 HCl + 6 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 | 18 | -18 HClO3 | 14 | -14 As_2S_3 | 3 | -3 H_2SO_4 | 9 | 9 HCl | 14 | 14 H_3AsO_4 | 6 | 6 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 | 18 | -18 | -1/18 (Δ[H2O])/(Δt) HClO3 | 14 | -14 | -1/14 (Δ[HClO3])/(Δt) As_2S_3 | 3 | -3 | -1/3 (Δ[As2S3])/(Δt) H_2SO_4 | 9 | 9 | 1/9 (Δ[H2SO4])/(Δt) HCl | 14 | 14 | 1/14 (Δ[HCl])/(Δt) H_3AsO_4 | 6 | 6 | 1/6 (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 = -1/18 (Δ[H2O])/(Δt) = -1/14 (Δ[HClO3])/(Δt) = -1/3 (Δ[As2S3])/(Δt) = 1/9 (Δ[H2SO4])/(Δt) = 1/14 (Δ[HCl])/(Δt) = 1/6 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | HClO3 | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid formula | H_2O | HClO3 | As_2S_3 | H_2SO_4 | HCl | H_3AsO_4 Hill formula | H_2O | HClO3 | As_2S_3 | H_2O_4S | ClH | AsH_3O_4 name | water | | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid IUPAC name | water | | | sulfuric acid | hydrogen chloride | arsoric acid
| water | HClO3 | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid formula | H_2O | HClO3 | As_2S_3 | H_2SO_4 | HCl | H_3AsO_4 Hill formula | H_2O | HClO3 | As_2S_3 | H_2O_4S | ClH | AsH_3O_4 name | water | | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid IUPAC name | water | | | sulfuric acid | hydrogen chloride | arsoric acid

Substance properties

| water | HClO3 | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid molar mass | 18.015 g/mol | 84.45 g/mol | 246 g/mol | 98.07 g/mol | 36.46 g/mol | 141.94 g/mol phase | liquid (at STP) | | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | | 300 °C | 10.371 °C | -114.17 °C | 35.5 °C boiling point | 99.9839 °C | | | 279.6 °C | -85 °C | 160 °C density | 1 g/cm^3 | | 3.43 g/cm^3 | 1.8305 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 2.2 g/cm^3 solubility in water | | | | very soluble | miscible | surface tension | 0.0728 N/m | | | 0.0735 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | 0.021 Pa s (at 25 °C) | | odor | odorless | | | odorless | |
| water | HClO3 | arsenic(III) sulfide | sulfuric acid | hydrogen chloride | arsenic acid, solid molar mass | 18.015 g/mol | 84.45 g/mol | 246 g/mol | 98.07 g/mol | 36.46 g/mol | 141.94 g/mol phase | liquid (at STP) | | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | | 300 °C | 10.371 °C | -114.17 °C | 35.5 °C boiling point | 99.9839 °C | | | 279.6 °C | -85 °C | 160 °C density | 1 g/cm^3 | | 3.43 g/cm^3 | 1.8305 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 2.2 g/cm^3 solubility in water | | | | very soluble | miscible | surface tension | 0.0728 N/m | | | 0.0735 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | 0.021 Pa s (at 25 °C) | | odor | odorless | | | odorless | |

Units

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