Fe + SnSO4 = FeSO4 + Sn

Fe iron + SnSO_4 stannous sulfate ⟶ FeSO_4 duretter + Sn white tin

Balance the chemical equation algebraically: Fe + SnSO_4 ⟶ FeSO_4 + Sn Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 SnSO_4 ⟶ c_3 FeSO_4 + c_4 Sn Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S and Sn: Fe: | c_1 = c_3 O: | 4 c_2 = 4 c_3 S: | c_2 = c_3 Sn: | 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: | | Fe + SnSO_4 ⟶ FeSO_4 + Sn

+ ⟶ +

iron + stannous sulfate ⟶ duretter + white tin

Construct the equilibrium constant, K, expression for: Fe + SnSO_4 ⟶ FeSO_4 + Sn 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: Fe + SnSO_4 ⟶ FeSO_4 + Sn 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 Fe | 1 | -1 SnSO_4 | 1 | -1 FeSO_4 | 1 | 1 Sn | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) SnSO_4 | 1 | -1 | ([SnSO4])^(-1) FeSO_4 | 1 | 1 | [FeSO4] Sn | 1 | 1 | [Sn] 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 = ([Fe])^(-1) ([SnSO4])^(-1) [FeSO4] [Sn] = ([FeSO4] [Sn])/([Fe] [SnSO4])

Construct the rate of reaction expression for: Fe + SnSO_4 ⟶ FeSO_4 + Sn 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: Fe + SnSO_4 ⟶ FeSO_4 + Sn 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 Fe | 1 | -1 SnSO_4 | 1 | -1 FeSO_4 | 1 | 1 Sn | 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 Fe | 1 | -1 | -(Δ[Fe])/(Δt) SnSO_4 | 1 | -1 | -(Δ[SnSO4])/(Δt) FeSO_4 | 1 | 1 | (Δ[FeSO4])/(Δt) Sn | 1 | 1 | (Δ[Sn])/(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[Fe])/(Δt) = -(Δ[SnSO4])/(Δt) = (Δ[FeSO4])/(Δt) = (Δ[Sn])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iron | stannous sulfate | duretter | white tin formula | Fe | SnSO_4 | FeSO_4 | Sn Hill formula | Fe | O_4SSn | FeO_4S | Sn name | iron | stannous sulfate | duretter | white tin IUPAC name | iron | tin(+2) cation sulfate | iron(+2) cation sulfate | tin

| iron | stannous sulfate | duretter | white tin molar mass | 55.845 g/mol | 214.77 g/mol | 151.9 g/mol | 118.71 g/mol phase | solid (at STP) | | | solid (at STP) melting point | 1535 °C | | | 231.9 °C boiling point | 2750 °C | | | 2602 °C density | 7.874 g/cm^3 | 4.15 g/cm^3 | 2.841 g/cm^3 | 7.31 g/cm^3 solubility in water | insoluble | soluble | | insoluble dynamic viscosity | | | | 0.001 Pa s (at 600 °C) odor | | | | odorless