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H2O + SO2 + HClO3 = H2SO4 + Cl2O

Input interpretation

H_2O water + SO_2 sulfur dioxide + HClO3 ⟶ H_2SO_4 sulfuric acid + Cl_2O chlorine monoxide
H_2O water + SO_2 sulfur dioxide + HClO3 ⟶ H_2SO_4 sulfuric acid + Cl_2O chlorine monoxide

Balanced equation

Balance the chemical equation algebraically: H_2O + SO_2 + HClO3 ⟶ H_2SO_4 + Cl_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 HClO3 ⟶ c_4 H_2SO_4 + c_5 Cl_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Cl: H: | 2 c_1 + c_3 = 2 c_4 O: | c_1 + 2 c_2 + 3 c_3 = 4 c_4 + c_5 S: | c_2 = c_4 Cl: | c_3 = 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 4 c_3 = 2 c_4 = 4 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + 4 SO_2 + 2 HClO3 ⟶ 4 H_2SO_4 + Cl_2O
Balance the chemical equation algebraically: H_2O + SO_2 + HClO3 ⟶ H_2SO_4 + Cl_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 HClO3 ⟶ c_4 H_2SO_4 + c_5 Cl_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Cl: H: | 2 c_1 + c_3 = 2 c_4 O: | c_1 + 2 c_2 + 3 c_3 = 4 c_4 + c_5 S: | c_2 = c_4 Cl: | c_3 = 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 4 c_3 = 2 c_4 = 4 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2O + 4 SO_2 + 2 HClO3 ⟶ 4 H_2SO_4 + Cl_2O

Structures

+ + HClO3 ⟶ +
+ + HClO3 ⟶ +

Names

water + sulfur dioxide + HClO3 ⟶ sulfuric acid + chlorine monoxide
water + sulfur dioxide + HClO3 ⟶ sulfuric acid + chlorine monoxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + SO_2 + HClO3 ⟶ H_2SO_4 + Cl_2O 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: 3 H_2O + 4 SO_2 + 2 HClO3 ⟶ 4 H_2SO_4 + Cl_2O 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 | 3 | -3 SO_2 | 4 | -4 HClO3 | 2 | -2 H_2SO_4 | 4 | 4 Cl_2O | 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 | 3 | -3 | ([H2O])^(-3) SO_2 | 4 | -4 | ([SO2])^(-4) HClO3 | 2 | -2 | ([HClO3])^(-2) H_2SO_4 | 4 | 4 | ([H2SO4])^4 Cl_2O | 1 | 1 | [Cl2O] 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])^(-3) ([SO2])^(-4) ([HClO3])^(-2) ([H2SO4])^4 [Cl2O] = (([H2SO4])^4 [Cl2O])/(([H2O])^3 ([SO2])^4 ([HClO3])^2)
Construct the equilibrium constant, K, expression for: H_2O + SO_2 + HClO3 ⟶ H_2SO_4 + Cl_2O 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: 3 H_2O + 4 SO_2 + 2 HClO3 ⟶ 4 H_2SO_4 + Cl_2O 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 | 3 | -3 SO_2 | 4 | -4 HClO3 | 2 | -2 H_2SO_4 | 4 | 4 Cl_2O | 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 | 3 | -3 | ([H2O])^(-3) SO_2 | 4 | -4 | ([SO2])^(-4) HClO3 | 2 | -2 | ([HClO3])^(-2) H_2SO_4 | 4 | 4 | ([H2SO4])^4 Cl_2O | 1 | 1 | [Cl2O] 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])^(-3) ([SO2])^(-4) ([HClO3])^(-2) ([H2SO4])^4 [Cl2O] = (([H2SO4])^4 [Cl2O])/(([H2O])^3 ([SO2])^4 ([HClO3])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2O + SO_2 + HClO3 ⟶ H_2SO_4 + Cl_2O 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: 3 H_2O + 4 SO_2 + 2 HClO3 ⟶ 4 H_2SO_4 + Cl_2O 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 | 3 | -3 SO_2 | 4 | -4 HClO3 | 2 | -2 H_2SO_4 | 4 | 4 Cl_2O | 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 | 3 | -3 | -1/3 (Δ[H2O])/(Δt) SO_2 | 4 | -4 | -1/4 (Δ[SO2])/(Δt) HClO3 | 2 | -2 | -1/2 (Δ[HClO3])/(Δt) H_2SO_4 | 4 | 4 | 1/4 (Δ[H2SO4])/(Δt) Cl_2O | 1 | 1 | (Δ[Cl2O])/(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 = -1/3 (Δ[H2O])/(Δt) = -1/4 (Δ[SO2])/(Δt) = -1/2 (Δ[HClO3])/(Δt) = 1/4 (Δ[H2SO4])/(Δt) = (Δ[Cl2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + SO_2 + HClO3 ⟶ H_2SO_4 + Cl_2O 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: 3 H_2O + 4 SO_2 + 2 HClO3 ⟶ 4 H_2SO_4 + Cl_2O 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 | 3 | -3 SO_2 | 4 | -4 HClO3 | 2 | -2 H_2SO_4 | 4 | 4 Cl_2O | 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 | 3 | -3 | -1/3 (Δ[H2O])/(Δt) SO_2 | 4 | -4 | -1/4 (Δ[SO2])/(Δt) HClO3 | 2 | -2 | -1/2 (Δ[HClO3])/(Δt) H_2SO_4 | 4 | 4 | 1/4 (Δ[H2SO4])/(Δt) Cl_2O | 1 | 1 | (Δ[Cl2O])/(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 = -1/3 (Δ[H2O])/(Δt) = -1/4 (Δ[SO2])/(Δt) = -1/2 (Δ[HClO3])/(Δt) = 1/4 (Δ[H2SO4])/(Δt) = (Δ[Cl2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | sulfur dioxide | HClO3 | sulfuric acid | chlorine monoxide formula | H_2O | SO_2 | HClO3 | H_2SO_4 | Cl_2O Hill formula | H_2O | O_2S | HClO3 | H_2O_4S | Cl_2O name | water | sulfur dioxide | | sulfuric acid | chlorine monoxide IUPAC name | water | sulfur dioxide | | sulfuric acid | chloro hypochlorite
| water | sulfur dioxide | HClO3 | sulfuric acid | chlorine monoxide formula | H_2O | SO_2 | HClO3 | H_2SO_4 | Cl_2O Hill formula | H_2O | O_2S | HClO3 | H_2O_4S | Cl_2O name | water | sulfur dioxide | | sulfuric acid | chlorine monoxide IUPAC name | water | sulfur dioxide | | sulfuric acid | chloro hypochlorite

Substance properties

| water | sulfur dioxide | HClO3 | sulfuric acid | chlorine monoxide molar mass | 18.015 g/mol | 64.06 g/mol | 84.45 g/mol | 98.07 g/mol | 86.9 g/mol phase | liquid (at STP) | gas (at STP) | | liquid (at STP) | gas (at STP) melting point | 0 °C | -73 °C | | 10.371 °C | -120.6 °C boiling point | 99.9839 °C | -10 °C | | 279.6 °C | 2.2 °C density | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | | 1.8305 g/cm^3 | 0.003552 g/cm^3 (at 20 °C) solubility in water | | | | very soluble | slightly 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 | HClO3 | sulfuric acid | chlorine monoxide molar mass | 18.015 g/mol | 64.06 g/mol | 84.45 g/mol | 98.07 g/mol | 86.9 g/mol phase | liquid (at STP) | gas (at STP) | | liquid (at STP) | gas (at STP) melting point | 0 °C | -73 °C | | 10.371 °C | -120.6 °C boiling point | 99.9839 °C | -10 °C | | 279.6 °C | 2.2 °C density | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | | 1.8305 g/cm^3 | 0.003552 g/cm^3 (at 20 °C) solubility in water | | | | very soluble | slightly 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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