H2O2 + ZnS = H2O + ZnSO4

H_2O_2 hydrogen peroxide + ZnS zinc sulfide ⟶ H_2O water + ZnSO_4 zinc sulfate

Balance the chemical equation algebraically: H_2O_2 + ZnS ⟶ H_2O + ZnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 ZnS ⟶ c_3 H_2O + c_4 ZnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Zn: H: | 2 c_1 = 2 c_3 O: | 2 c_1 = c_3 + 4 c_4 S: | c_2 = c_4 Zn: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 4 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O_2 + ZnS ⟶ 4 H_2O + ZnSO_4

+ ⟶ +

hydrogen peroxide + zinc sulfide ⟶ water + zinc sulfate

Construct the equilibrium constant, K, expression for: H_2O_2 + ZnS ⟶ H_2O + 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: 4 H_2O_2 + ZnS ⟶ 4 H_2O + 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 H_2O_2 | 4 | -4 ZnS | 1 | -1 H_2O | 4 | 4 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 H_2O_2 | 4 | -4 | ([H2O2])^(-4) ZnS | 1 | -1 | ([ZnS])^(-1) H_2O | 4 | 4 | ([H2O])^4 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 = ([H2O2])^(-4) ([ZnS])^(-1) ([H2O])^4 [ZnSO4] = (([H2O])^4 [ZnSO4])/(([H2O2])^4 [ZnS])

Construct the rate of reaction expression for: H_2O_2 + ZnS ⟶ H_2O + 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: 4 H_2O_2 + ZnS ⟶ 4 H_2O + 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 H_2O_2 | 4 | -4 ZnS | 1 | -1 H_2O | 4 | 4 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 H_2O_2 | 4 | -4 | -1/4 (Δ[H2O2])/(Δt) ZnS | 1 | -1 | -(Δ[ZnS])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(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 = -1/4 (Δ[H2O2])/(Δt) = -(Δ[ZnS])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[ZnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen peroxide | zinc sulfide | water | zinc sulfate formula | H_2O_2 | ZnS | H_2O | ZnSO_4 Hill formula | H_2O_2 | SZn | H_2O | O_4SZn name | hydrogen peroxide | zinc sulfide | water | zinc sulfate IUPAC name | hydrogen peroxide | thioxozinc | water | zinc sulfate

| hydrogen peroxide | zinc sulfide | water | zinc sulfate molar mass | 34.014 g/mol | 97.44 g/mol | 18.015 g/mol | 161.4 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | melting point | -0.43 °C | 1064 °C | 0 °C | boiling point | 150.2 °C | | 99.9839 °C | density | 1.44 g/cm^3 | 4.1 g/cm^3 | 1 g/cm^3 | 1.005 g/cm^3 solubility in water | miscible | | | soluble surface tension | 0.0804 N/m | | 0.0728 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless | odorless