CuSO4 + Sn = Cu + SnSO4

CuSO_4 copper(II) sulfate + Sn white tin ⟶ Cu copper + SnSO_4 stannous sulfate

Balance the chemical equation algebraically: CuSO_4 + Sn ⟶ Cu + SnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuSO_4 + c_2 Sn ⟶ c_3 Cu + c_4 SnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, S and Sn: Cu: | c_1 = c_3 O: | 4 c_1 = 4 c_4 S: | c_1 = c_4 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: | | CuSO_4 + Sn ⟶ Cu + SnSO_4

+ ⟶ +

copper(II) sulfate + white tin ⟶ copper + stannous sulfate

Construct the equilibrium constant, K, expression for: CuSO_4 + Sn ⟶ Cu + SnSO_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: CuSO_4 + Sn ⟶ Cu + SnSO_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 CuSO_4 | 1 | -1 Sn | 1 | -1 Cu | 1 | 1 SnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuSO_4 | 1 | -1 | ([CuSO4])^(-1) Sn | 1 | -1 | ([Sn])^(-1) Cu | 1 | 1 | [Cu] SnSO_4 | 1 | 1 | [SnSO4] 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 = ([CuSO4])^(-1) ([Sn])^(-1) [Cu] [SnSO4] = ([Cu] [SnSO4])/([CuSO4] [Sn])

Construct the rate of reaction expression for: CuSO_4 + Sn ⟶ Cu + SnSO_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: CuSO_4 + Sn ⟶ Cu + SnSO_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 CuSO_4 | 1 | -1 Sn | 1 | -1 Cu | 1 | 1 SnSO_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 CuSO_4 | 1 | -1 | -(Δ[CuSO4])/(Δt) Sn | 1 | -1 | -(Δ[Sn])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(Δt) SnSO_4 | 1 | 1 | (Δ[SnSO4])/(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[CuSO4])/(Δt) = -(Δ[Sn])/(Δt) = (Δ[Cu])/(Δt) = (Δ[SnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper(II) sulfate | white tin | copper | stannous sulfate formula | CuSO_4 | Sn | Cu | SnSO_4 Hill formula | CuO_4S | Sn | Cu | O_4SSn name | copper(II) sulfate | white tin | copper | stannous sulfate IUPAC name | copper sulfate | tin | copper | tin(+2) cation sulfate

| copper(II) sulfate | white tin | copper | stannous sulfate molar mass | 159.6 g/mol | 118.71 g/mol | 63.546 g/mol | 214.77 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 200 °C | 231.9 °C | 1083 °C | boiling point | | 2602 °C | 2567 °C | density | 3.603 g/cm^3 | 7.31 g/cm^3 | 8.96 g/cm^3 | 4.15 g/cm^3 solubility in water | | insoluble | insoluble | soluble dynamic viscosity | | 0.001 Pa s (at 600 °C) | | odor | | odorless | odorless |