H2SO4 + SrSO3 = H2SO3 + SrSO4

H_2SO_4 sulfuric acid + SrSO3 ⟶ H_2SO_3 sulfurous acid + SrSO_4 strontium sulfate

Balance the chemical equation algebraically: H_2SO_4 + SrSO3 ⟶ H_2SO_3 + SrSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 SrSO3 ⟶ c_3 H_2SO_3 + c_4 SrSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Sr: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 3 c_2 = 3 c_3 + 4 c_4 S: | c_1 + c_2 = c_3 + c_4 Sr: | c_2 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + SrSO3 ⟶ H_2SO_3 + SrSO_4

+ SrSO3 ⟶ +

sulfuric acid + SrSO3 ⟶ sulfurous acid + strontium sulfate

Construct the equilibrium constant, K, expression for: H_2SO_4 + SrSO3 ⟶ H_2SO_3 + SrSO_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: H_2SO_4 + SrSO3 ⟶ H_2SO_3 + SrSO_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_2SO_4 | 1 | -1 SrSO3 | 1 | -1 H_2SO_3 | 1 | 1 SrSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) SrSO3 | 1 | -1 | ([SrSO3])^(-1) H_2SO_3 | 1 | 1 | [H2SO3] SrSO_4 | 1 | 1 | [SrSO4] 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 = ([H2SO4])^(-1) ([SrSO3])^(-1) [H2SO3] [SrSO4] = ([H2SO3] [SrSO4])/([H2SO4] [SrSO3])

Construct the rate of reaction expression for: H_2SO_4 + SrSO3 ⟶ H_2SO_3 + SrSO_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: H_2SO_4 + SrSO3 ⟶ H_2SO_3 + SrSO_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_2SO_4 | 1 | -1 SrSO3 | 1 | -1 H_2SO_3 | 1 | 1 SrSO_4 | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) SrSO3 | 1 | -1 | -(Δ[SrSO3])/(Δt) H_2SO_3 | 1 | 1 | (Δ[H2SO3])/(Δt) SrSO_4 | 1 | 1 | (Δ[SrSO4])/(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[H2SO4])/(Δt) = -(Δ[SrSO3])/(Δt) = (Δ[H2SO3])/(Δt) = (Δ[SrSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | SrSO3 | sulfurous acid | strontium sulfate formula | H_2SO_4 | SrSO3 | H_2SO_3 | SrSO_4 Hill formula | H_2O_4S | O3SSr | H_2O_3S | O_4SSr name | sulfuric acid | | sulfurous acid | strontium sulfate

| sulfuric acid | SrSO3 | sulfurous acid | strontium sulfate molar mass | 98.07 g/mol | 167.7 g/mol | 82.07 g/mol | 183.7 g/mol phase | liquid (at STP) | | | solid (at STP) melting point | 10.371 °C | | | 1605 °C boiling point | 279.6 °C | | | density | 1.8305 g/cm^3 | | 1.03 g/cm^3 | 3.96 g/cm^3 solubility in water | very soluble | | very soluble | surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | odor | odorless | | |