ZnSO4 + BaS = BaSO4 + ZnS

ZnSO_4 zinc sulfate + BaS barium sulfide ⟶ BaSO_4 barium sulfate + ZnS zinc sulfide

Balance the chemical equation algebraically: ZnSO_4 + BaS ⟶ BaSO_4 + ZnS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ZnSO_4 + c_2 BaS ⟶ c_3 BaSO_4 + c_4 ZnS Set the number of atoms in the reactants equal to the number of atoms in the products for O, S, Zn and Ba: O: | 4 c_1 = 4 c_3 S: | c_1 + c_2 = c_3 + c_4 Zn: | c_1 = c_4 Ba: | 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: | | ZnSO_4 + BaS ⟶ BaSO_4 + ZnS

+ ⟶ +

zinc sulfate + barium sulfide ⟶ barium sulfate + zinc sulfide

Construct the equilibrium constant, K, expression for: ZnSO_4 + BaS ⟶ BaSO_4 + ZnS 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: ZnSO_4 + BaS ⟶ BaSO_4 + ZnS 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 ZnSO_4 | 1 | -1 BaS | 1 | -1 BaSO_4 | 1 | 1 ZnS | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression ZnSO_4 | 1 | -1 | ([ZnSO4])^(-1) BaS | 1 | -1 | ([BaS])^(-1) BaSO_4 | 1 | 1 | [BaSO4] ZnS | 1 | 1 | [ZnS] 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 = ([ZnSO4])^(-1) ([BaS])^(-1) [BaSO4] [ZnS] = ([BaSO4] [ZnS])/([ZnSO4] [BaS])

Construct the rate of reaction expression for: ZnSO_4 + BaS ⟶ BaSO_4 + ZnS 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: ZnSO_4 + BaS ⟶ BaSO_4 + ZnS 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 ZnSO_4 | 1 | -1 BaS | 1 | -1 BaSO_4 | 1 | 1 ZnS | 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 ZnSO_4 | 1 | -1 | -(Δ[ZnSO4])/(Δt) BaS | 1 | -1 | -(Δ[BaS])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(Δt) ZnS | 1 | 1 | (Δ[ZnS])/(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[ZnSO4])/(Δt) = -(Δ[BaS])/(Δt) = (Δ[BaSO4])/(Δt) = (Δ[ZnS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| zinc sulfate | barium sulfide | barium sulfate | zinc sulfide formula | ZnSO_4 | BaS | BaSO_4 | ZnS Hill formula | O_4SZn | BaS | BaO_4S | SZn name | zinc sulfate | barium sulfide | barium sulfate | zinc sulfide IUPAC name | zinc sulfate | thioxobarium | barium(+2) cation sulfate | thioxozinc

| zinc sulfate | barium sulfide | barium sulfate | zinc sulfide molar mass | 161.4 g/mol | 169.39 g/mol | 233.38 g/mol | 97.44 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 1999.85 °C | 1345 °C | 1064 °C density | 1.005 g/cm^3 | 4.25 g/cm^3 | 4.5 g/cm^3 | 4.1 g/cm^3 solubility in water | soluble | | insoluble | odor | odorless | | |