H2SO4 + Cu = CuO + SO2H2O

H_2SO_4 sulfuric acid + Cu copper ⟶ CuO cupric oxide + H_2SO_3 sulfurous acid

Balance the chemical equation algebraically: H_2SO_4 + Cu ⟶ CuO + H_2SO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Cu ⟶ c_3 CuO + c_4 H_2SO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Cu: H: | 2 c_1 = 2 c_4 O: | 4 c_1 = c_3 + 3 c_4 S: | c_1 = c_4 Cu: | 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_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 + Cu ⟶ CuO + H_2SO_3

+ ⟶ +

sulfuric acid + copper ⟶ cupric oxide + sulfurous acid

Construct the equilibrium constant, K, expression for: H_2SO_4 + Cu ⟶ CuO + H_2SO_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_2SO_4 + Cu ⟶ CuO + H_2SO_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_2SO_4 | 1 | -1 Cu | 1 | -1 CuO | 1 | 1 H_2SO_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_2SO_4 | 1 | -1 | ([H2SO4])^(-1) Cu | 1 | -1 | ([Cu])^(-1) CuO | 1 | 1 | [CuO] H_2SO_3 | 1 | 1 | [H2SO3] 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) ([Cu])^(-1) [CuO] [H2SO3] = ([CuO] [H2SO3])/([H2SO4] [Cu])

Construct the rate of reaction expression for: H_2SO_4 + Cu ⟶ CuO + H_2SO_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_2SO_4 + Cu ⟶ CuO + H_2SO_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_2SO_4 | 1 | -1 Cu | 1 | -1 CuO | 1 | 1 H_2SO_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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) Cu | 1 | -1 | -(Δ[Cu])/(Δt) CuO | 1 | 1 | (Δ[CuO])/(Δt) H_2SO_3 | 1 | 1 | (Δ[H2SO3])/(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[Cu])/(Δt) = (Δ[CuO])/(Δt) = (Δ[H2SO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | copper | cupric oxide | sulfurous acid formula | H_2SO_4 | Cu | CuO | H_2SO_3 Hill formula | H_2O_4S | Cu | CuO | H_2O_3S name | sulfuric acid | copper | cupric oxide | sulfurous acid