O2 + ZnS = ZnSO4

O_2 oxygen + ZnS zinc sulfide ⟶ ZnSO_4 zinc sulfate

Balance the chemical equation algebraically: O_2 + ZnS ⟶ ZnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 ZnS ⟶ c_3 ZnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S and Zn: O: | 2 c_1 = 4 c_3 S: | c_2 = c_3 Zn: | 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 O_2 + ZnS ⟶ ZnSO_4

+ ⟶

oxygen + zinc sulfide ⟶ zinc sulfate

Construct the equilibrium constant, K, expression for: O_2 + ZnS ⟶ ZnSO_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: 2 O_2 + ZnS ⟶ ZnSO_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 O_2 | 2 | -2 ZnS | 1 | -1 ZnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 2 | -2 | ([O2])^(-2) ZnS | 1 | -1 | ([ZnS])^(-1) ZnSO_4 | 1 | 1 | [ZnSO4] 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 = ([O2])^(-2) ([ZnS])^(-1) [ZnSO4] = ([ZnSO4])/(([O2])^2 [ZnS])

Construct the rate of reaction expression for: O_2 + ZnS ⟶ ZnSO_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: 2 O_2 + ZnS ⟶ ZnSO_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 O_2 | 2 | -2 ZnS | 1 | -1 ZnSO_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 O_2 | 2 | -2 | -1/2 (Δ[O2])/(Δt) ZnS | 1 | -1 | -(Δ[ZnS])/(Δt) ZnSO_4 | 1 | 1 | (Δ[ZnSO4])/(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[O2])/(Δt) = -(Δ[ZnS])/(Δt) = (Δ[ZnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| oxygen | zinc sulfide | zinc sulfate formula | O_2 | ZnS | ZnSO_4 Hill formula | O_2 | SZn | O_4SZn name | oxygen | zinc sulfide | zinc sulfate IUPAC name | molecular oxygen | thioxozinc | zinc sulfate

| oxygen | zinc sulfide | zinc sulfate molar mass | 31.998 g/mol | 97.44 g/mol | 161.4 g/mol phase | gas (at STP) | solid (at STP) | melting point | -218 °C | 1064 °C | boiling point | -183 °C | | density | 0.001429 g/cm^3 (at 0 °C) | 4.1 g/cm^3 | 1.005 g/cm^3 solubility in water | | | soluble surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | | odorless