CuO + H2SO3 = H2O + CuSO3

CuO cupric oxide + H_2SO_3 sulfurous acid ⟶ H_2O water + CuSO3

Balance the chemical equation algebraically: CuO + H_2SO_3 ⟶ H_2O + CuSO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 H_2SO_3 ⟶ c_3 H_2O + c_4 CuSO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, H and S: Cu: | c_1 = c_4 O: | c_1 + 3 c_2 = c_3 + 3 c_4 H: | 2 c_2 = 2 c_3 S: | 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: | | CuO + H_2SO_3 ⟶ H_2O + CuSO3

+ ⟶ + CuSO3

cupric oxide + sulfurous acid ⟶ water + CuSO3

Construct the equilibrium constant, K, expression for: CuO + H_2SO_3 ⟶ H_2O + CuSO3 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: CuO + H_2SO_3 ⟶ H_2O + CuSO3 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 CuO | 1 | -1 H_2SO_3 | 1 | -1 H_2O | 1 | 1 CuSO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 1 | -1 | ([CuO])^(-1) H_2SO_3 | 1 | -1 | ([H2SO3])^(-1) H_2O | 1 | 1 | [H2O] CuSO3 | 1 | 1 | [CuSO3] 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 = ([CuO])^(-1) ([H2SO3])^(-1) [H2O] [CuSO3] = ([H2O] [CuSO3])/([CuO] [H2SO3])

Construct the rate of reaction expression for: CuO + H_2SO_3 ⟶ H_2O + CuSO3 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: CuO + H_2SO_3 ⟶ H_2O + CuSO3 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 CuO | 1 | -1 H_2SO_3 | 1 | -1 H_2O | 1 | 1 CuSO3 | 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 CuO | 1 | -1 | -(Δ[CuO])/(Δt) H_2SO_3 | 1 | -1 | -(Δ[H2SO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CuSO3 | 1 | 1 | (Δ[CuSO3])/(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[CuO])/(Δt) = -(Δ[H2SO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CuSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| cupric oxide | sulfurous acid | water | CuSO3 formula | CuO | H_2SO_3 | H_2O | CuSO3 Hill formula | CuO | H_2O_3S | H_2O | CuO3S name | cupric oxide | sulfurous acid | water |

| cupric oxide | sulfurous acid | water | CuSO3 molar mass | 79.545 g/mol | 82.07 g/mol | 18.015 g/mol | 143.6 g/mol phase | solid (at STP) | | liquid (at STP) | melting point | 1326 °C | | 0 °C | boiling point | 2000 °C | | 99.9839 °C | density | 6.315 g/cm^3 | 1.03 g/cm^3 | 1 g/cm^3 | solubility in water | insoluble | very soluble | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |