Sn + Cu(NO3) = Cu + Sn(NO3)4

Sn white tin + Cu(NO_3)_2 copper(II) nitrate ⟶ Cu copper + Sn(NO3)4

Balance the chemical equation algebraically: Sn + Cu(NO_3)_2 ⟶ Cu + Sn(NO3)4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Sn + c_2 Cu(NO_3)_2 ⟶ c_3 Cu + c_4 Sn(NO3)4 Set the number of atoms in the reactants equal to the number of atoms in the products for Sn, Cu, N and O: Sn: | c_1 = c_4 Cu: | c_2 = c_3 N: | 2 c_2 = 4 c_4 O: | 6 c_2 = 12 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Sn + 2 Cu(NO_3)_2 ⟶ 2 Cu + Sn(NO3)4

+ ⟶ + Sn(NO3)4

white tin + copper(II) nitrate ⟶ copper + Sn(NO3)4

Construct the equilibrium constant, K, expression for: Sn + Cu(NO_3)_2 ⟶ Cu + Sn(NO3)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: Sn + 2 Cu(NO_3)_2 ⟶ 2 Cu + Sn(NO3)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 Sn | 1 | -1 Cu(NO_3)_2 | 2 | -2 Cu | 2 | 2 Sn(NO3)4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Sn | 1 | -1 | ([Sn])^(-1) Cu(NO_3)_2 | 2 | -2 | ([Cu(NO3)2])^(-2) Cu | 2 | 2 | ([Cu])^2 Sn(NO3)4 | 1 | 1 | [Sn(NO3)4] 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 = ([Sn])^(-1) ([Cu(NO3)2])^(-2) ([Cu])^2 [Sn(NO3)4] = (([Cu])^2 [Sn(NO3)4])/([Sn] ([Cu(NO3)2])^2)

Construct the rate of reaction expression for: Sn + Cu(NO_3)_2 ⟶ Cu + Sn(NO3)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: Sn + 2 Cu(NO_3)_2 ⟶ 2 Cu + Sn(NO3)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 Sn | 1 | -1 Cu(NO_3)_2 | 2 | -2 Cu | 2 | 2 Sn(NO3)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 Sn | 1 | -1 | -(Δ[Sn])/(Δt) Cu(NO_3)_2 | 2 | -2 | -1/2 (Δ[Cu(NO3)2])/(Δt) Cu | 2 | 2 | 1/2 (Δ[Cu])/(Δt) Sn(NO3)4 | 1 | 1 | (Δ[Sn(NO3)4])/(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[Sn])/(Δt) = -1/2 (Δ[Cu(NO3)2])/(Δt) = 1/2 (Δ[Cu])/(Δt) = (Δ[Sn(NO3)4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| white tin | copper(II) nitrate | copper | Sn(NO3)4 formula | Sn | Cu(NO_3)_2 | Cu | Sn(NO3)4 Hill formula | Sn | CuN_2O_6 | Cu | N4O12Sn name | white tin | copper(II) nitrate | copper | IUPAC name | tin | copper(II) nitrate | copper |

| white tin | copper(II) nitrate | copper | Sn(NO3)4 molar mass | 118.71 g/mol | 187.55 g/mol | 63.546 g/mol | 366.73 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 231.9 °C | | 1083 °C | boiling point | 2602 °C | | 2567 °C | density | 7.31 g/cm^3 | | 8.96 g/cm^3 | solubility in water | insoluble | | insoluble | dynamic viscosity | 0.001 Pa s (at 600 °C) | | | odor | odorless | | odorless |