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H2O + H2S2O8 = H2SO4 + H2O2

Input interpretation

H_2O water + H2S2O8 ⟶ H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide
H_2O water + H2S2O8 ⟶ H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide

Balanced equation

Balance the chemical equation algebraically: H_2O + H2S2O8 ⟶ H_2SO_4 + H_2O_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 H2S2O8 ⟶ c_3 H_2SO_4 + c_4 H_2O_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and S: H: | 2 c_1 + 2 c_2 = 2 c_3 + 2 c_4 O: | c_1 + 8 c_2 = 4 c_3 + 2 c_4 S: | 2 c_2 = c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + H2S2O8 ⟶ 2 H_2SO_4 + H_2O_2
Balance the chemical equation algebraically: H_2O + H2S2O8 ⟶ H_2SO_4 + H_2O_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 H2S2O8 ⟶ c_3 H_2SO_4 + c_4 H_2O_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and S: H: | 2 c_1 + 2 c_2 = 2 c_3 + 2 c_4 O: | c_1 + 8 c_2 = 4 c_3 + 2 c_4 S: | 2 c_2 = c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + H2S2O8 ⟶ 2 H_2SO_4 + H_2O_2

Structures

+ H2S2O8 ⟶ +
+ H2S2O8 ⟶ +

Names

water + H2S2O8 ⟶ sulfuric acid + hydrogen peroxide
water + H2S2O8 ⟶ sulfuric acid + hydrogen peroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + H2S2O8 ⟶ H_2SO_4 + H_2O_2 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: 2 H_2O + H2S2O8 ⟶ 2 H_2SO_4 + H_2O_2 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 | 2 | -2 H2S2O8 | 1 | -1 H_2SO_4 | 2 | 2 H_2O_2 | 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 | 2 | -2 | ([H2O])^(-2) H2S2O8 | 1 | -1 | ([H2S2O8])^(-1) H_2SO_4 | 2 | 2 | ([H2SO4])^2 H_2O_2 | 1 | 1 | [H2O2] 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])^(-2) ([H2S2O8])^(-1) ([H2SO4])^2 [H2O2] = (([H2SO4])^2 [H2O2])/(([H2O])^2 [H2S2O8])
Construct the equilibrium constant, K, expression for: H_2O + H2S2O8 ⟶ H_2SO_4 + H_2O_2 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: 2 H_2O + H2S2O8 ⟶ 2 H_2SO_4 + H_2O_2 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 | 2 | -2 H2S2O8 | 1 | -1 H_2SO_4 | 2 | 2 H_2O_2 | 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 | 2 | -2 | ([H2O])^(-2) H2S2O8 | 1 | -1 | ([H2S2O8])^(-1) H_2SO_4 | 2 | 2 | ([H2SO4])^2 H_2O_2 | 1 | 1 | [H2O2] 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])^(-2) ([H2S2O8])^(-1) ([H2SO4])^2 [H2O2] = (([H2SO4])^2 [H2O2])/(([H2O])^2 [H2S2O8])

Rate of reaction

Construct the rate of reaction expression for: H_2O + H2S2O8 ⟶ H_2SO_4 + H_2O_2 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: 2 H_2O + H2S2O8 ⟶ 2 H_2SO_4 + H_2O_2 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 | 2 | -2 H2S2O8 | 1 | -1 H_2SO_4 | 2 | 2 H_2O_2 | 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 | 2 | -2 | -1/2 (Δ[H2O])/(Δt) H2S2O8 | 1 | -1 | -(Δ[H2S2O8])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) H_2O_2 | 1 | 1 | (Δ[H2O2])/(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 = -1/2 (Δ[H2O])/(Δt) = -(Δ[H2S2O8])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = (Δ[H2O2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + H2S2O8 ⟶ H_2SO_4 + H_2O_2 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: 2 H_2O + H2S2O8 ⟶ 2 H_2SO_4 + H_2O_2 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 | 2 | -2 H2S2O8 | 1 | -1 H_2SO_4 | 2 | 2 H_2O_2 | 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 | 2 | -2 | -1/2 (Δ[H2O])/(Δt) H2S2O8 | 1 | -1 | -(Δ[H2S2O8])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) H_2O_2 | 1 | 1 | (Δ[H2O2])/(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 = -1/2 (Δ[H2O])/(Δt) = -(Δ[H2S2O8])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = (Δ[H2O2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | H2S2O8 | sulfuric acid | hydrogen peroxide formula | H_2O | H2S2O8 | H_2SO_4 | H_2O_2 Hill formula | H_2O | H2O8S2 | H_2O_4S | H_2O_2 name | water | | sulfuric acid | hydrogen peroxide
| water | H2S2O8 | sulfuric acid | hydrogen peroxide formula | H_2O | H2S2O8 | H_2SO_4 | H_2O_2 Hill formula | H_2O | H2O8S2 | H_2O_4S | H_2O_2 name | water | | sulfuric acid | hydrogen peroxide

Substance properties

| water | H2S2O8 | sulfuric acid | hydrogen peroxide molar mass | 18.015 g/mol | 194.1 g/mol | 98.07 g/mol | 34.014 g/mol phase | liquid (at STP) | | liquid (at STP) | liquid (at STP) melting point | 0 °C | | 10.371 °C | -0.43 °C boiling point | 99.9839 °C | | 279.6 °C | 150.2 °C density | 1 g/cm^3 | | 1.8305 g/cm^3 | 1.44 g/cm^3 solubility in water | | | very soluble | miscible surface tension | 0.0728 N/m | | 0.0735 N/m | 0.0804 N/m dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | 0.001249 Pa s (at 20 °C) odor | odorless | | odorless |
| water | H2S2O8 | sulfuric acid | hydrogen peroxide molar mass | 18.015 g/mol | 194.1 g/mol | 98.07 g/mol | 34.014 g/mol phase | liquid (at STP) | | liquid (at STP) | liquid (at STP) melting point | 0 °C | | 10.371 °C | -0.43 °C boiling point | 99.9839 °C | | 279.6 °C | 150.2 °C density | 1 g/cm^3 | | 1.8305 g/cm^3 | 1.44 g/cm^3 solubility in water | | | very soluble | miscible surface tension | 0.0728 N/m | | 0.0735 N/m | 0.0804 N/m dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | 0.001249 Pa s (at 20 °C) odor | odorless | | odorless |

Units

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