H2SO4Na2S = H2SNa2SO4

H2SO4Na2S ⟶ H2SNa2SO4

Balance the chemical equation algebraically: H2SO4Na2S ⟶ H2SNa2SO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H2SO4Na2S ⟶ c_2 H2SNa2SO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, O and Na: H: | 2 c_1 = 2 c_2 S: | 2 c_1 = 2 c_2 O: | 4 c_1 = 4 c_2 Na: | 2 c_1 = 2 c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H2SO4Na2S ⟶ H2SNa2SO4

H2SO4Na2S ⟶ H2SNa2SO4

H2SO4Na2S ⟶ H2SNa2SO4

Construct the equilibrium constant, K, expression for: H2SO4Na2S ⟶ H2SNa2SO4 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: H2SO4Na2S ⟶ H2SNa2SO4 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 H2SO4Na2S | 1 | -1 H2SNa2SO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H2SO4Na2S | 1 | -1 | ([H2SO4Na2S])^(-1) H2SNa2SO4 | 1 | 1 | [H2SNa2SO4] 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 = ([H2SO4Na2S])^(-1) [H2SNa2SO4] = ([H2SNa2SO4])/([H2SO4Na2S])

Construct the rate of reaction expression for: H2SO4Na2S ⟶ H2SNa2SO4 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: H2SO4Na2S ⟶ H2SNa2SO4 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 H2SO4Na2S | 1 | -1 H2SNa2SO4 | 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 H2SO4Na2S | 1 | -1 | -(Δ[H2SO4Na2S])/(Δt) H2SNa2SO4 | 1 | 1 | (Δ[H2SNa2SO4])/(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[H2SO4Na2S])/(Δt) = (Δ[H2SNa2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| H2SO4Na2S | H2SNa2SO4 formula | H2SO4Na2S | H2SNa2SO4 Hill formula | H2Na2O4S2 | H2Na2O4S2

| H2SO4Na2S | H2SNa2SO4 molar mass | 176.1 g/mol | 176.1 g/mol