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H2O + SO2 + H3AsO4 = H2SO4 + H3AsO3

Input interpretation

H_2O water + SO_2 sulfur dioxide + H_3AsO_4 arsenic acid, solid ⟶ H_2SO_4 sulfuric acid + As(OH)_3 arsenious acid
H_2O water + SO_2 sulfur dioxide + H_3AsO_4 arsenic acid, solid ⟶ H_2SO_4 sulfuric acid + As(OH)_3 arsenious acid

Balanced equation

Balance the chemical equation algebraically: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 H_3AsO_4 ⟶ c_4 H_2SO_4 + c_5 As(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and As: H: | 2 c_1 + 3 c_3 = 2 c_4 + 3 c_5 O: | c_1 + 2 c_2 + 4 c_3 = 4 c_4 + 3 c_5 S: | c_2 = c_4 As: | 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 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_3
Balance the chemical equation algebraically: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 H_3AsO_4 ⟶ c_4 H_2SO_4 + c_5 As(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and As: H: | 2 c_1 + 3 c_3 = 2 c_4 + 3 c_5 O: | c_1 + 2 c_2 + 4 c_3 = 4 c_4 + 3 c_5 S: | c_2 = c_4 As: | 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 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_3

Structures

+ + ⟶ +
+ + ⟶ +

Names

water + sulfur dioxide + arsenic acid, solid ⟶ sulfuric acid + arsenious acid
water + sulfur dioxide + arsenic acid, solid ⟶ sulfuric acid + arsenious acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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 H_2O | 1 | -1 SO_2 | 1 | -1 H_3AsO_4 | 1 | -1 H_2SO_4 | 1 | 1 As(OH)_3 | 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) SO_2 | 1 | -1 | ([SO2])^(-1) H_3AsO_4 | 1 | -1 | ([H3AsO4])^(-1) H_2SO_4 | 1 | 1 | [H2SO4] As(OH)_3 | 1 | 1 | [As(OH)3] 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) ([SO2])^(-1) ([H3AsO4])^(-1) [H2SO4] [As(OH)3] = ([H2SO4] [As(OH)3])/([H2O] [SO2] [H3AsO4])
Construct the equilibrium constant, K, expression for: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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 H_2O | 1 | -1 SO_2 | 1 | -1 H_3AsO_4 | 1 | -1 H_2SO_4 | 1 | 1 As(OH)_3 | 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) SO_2 | 1 | -1 | ([SO2])^(-1) H_3AsO_4 | 1 | -1 | ([H3AsO4])^(-1) H_2SO_4 | 1 | 1 | [H2SO4] As(OH)_3 | 1 | 1 | [As(OH)3] 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) ([SO2])^(-1) ([H3AsO4])^(-1) [H2SO4] [As(OH)3] = ([H2SO4] [As(OH)3])/([H2O] [SO2] [H3AsO4])

Rate of reaction

Construct the rate of reaction expression for: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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 H_2O | 1 | -1 SO_2 | 1 | -1 H_3AsO_4 | 1 | -1 H_2SO_4 | 1 | 1 As(OH)_3 | 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) SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) H_3AsO_4 | 1 | -1 | -(Δ[H3AsO4])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) As(OH)_3 | 1 | 1 | (Δ[As(OH)3])/(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[SO2])/(Δt) = -(Δ[H3AsO4])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[As(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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: H_2O + SO_2 + H_3AsO_4 ⟶ H_2SO_4 + As(OH)_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 H_2O | 1 | -1 SO_2 | 1 | -1 H_3AsO_4 | 1 | -1 H_2SO_4 | 1 | 1 As(OH)_3 | 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) SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) H_3AsO_4 | 1 | -1 | -(Δ[H3AsO4])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) As(OH)_3 | 1 | 1 | (Δ[As(OH)3])/(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[SO2])/(Δt) = -(Δ[H3AsO4])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[As(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | sulfur dioxide | arsenic acid, solid | sulfuric acid | arsenious acid formula | H_2O | SO_2 | H_3AsO_4 | H_2SO_4 | As(OH)_3 Hill formula | H_2O | O_2S | AsH_3O_4 | H_2O_4S | AsH_3O_3 name | water | sulfur dioxide | arsenic acid, solid | sulfuric acid | arsenious acid IUPAC name | water | sulfur dioxide | arsoric acid | sulfuric acid | arsorous acid
| water | sulfur dioxide | arsenic acid, solid | sulfuric acid | arsenious acid formula | H_2O | SO_2 | H_3AsO_4 | H_2SO_4 | As(OH)_3 Hill formula | H_2O | O_2S | AsH_3O_4 | H_2O_4S | AsH_3O_3 name | water | sulfur dioxide | arsenic acid, solid | sulfuric acid | arsenious acid IUPAC name | water | sulfur dioxide | arsoric acid | sulfuric acid | arsorous acid

Substance properties

| water | sulfur dioxide | arsenic acid, solid | sulfuric acid | arsenious acid molar mass | 18.015 g/mol | 64.06 g/mol | 141.94 g/mol | 98.07 g/mol | 125.94 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 0 °C | -73 °C | 35.5 °C | 10.371 °C | boiling point | 99.9839 °C | -10 °C | 160 °C | 279.6 °C | density | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 2.2 g/cm^3 | 1.8305 g/cm^3 | solubility in water | | | | very soluble | surface tension | 0.0728 N/m | 0.02859 N/m | | 0.0735 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | odor | odorless | | | odorless |
| water | sulfur dioxide | arsenic acid, solid | sulfuric acid | arsenious acid molar mass | 18.015 g/mol | 64.06 g/mol | 141.94 g/mol | 98.07 g/mol | 125.94 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 0 °C | -73 °C | 35.5 °C | 10.371 °C | boiling point | 99.9839 °C | -10 °C | 160 °C | 279.6 °C | density | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 2.2 g/cm^3 | 1.8305 g/cm^3 | solubility in water | | | | very soluble | surface tension | 0.0728 N/m | 0.02859 N/m | | 0.0735 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | odor | odorless | | | odorless |

Units

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