SnCl2AgNO3 = SnNO3AgCl2

SnCl2AgNO3 ⟶ SnNO3AgCl2

Balance the chemical equation algebraically: SnCl2AgNO3 ⟶ SnNO3AgCl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnCl2AgNO3 ⟶ c_2 SnNO3AgCl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Sn, Cl, Ag, N and O: Sn: | c_1 = c_2 Cl: | 2 c_1 = 2 c_2 Ag: | c_1 = c_2 N: | c_1 = c_2 O: | 3 c_1 = 3 c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SnCl2AgNO3 ⟶ SnNO3AgCl2

SnCl2AgNO3 ⟶ SnNO3AgCl2

SnCl2AgNO3 ⟶ SnNO3AgCl2

Construct the equilibrium constant, K, expression for: SnCl2AgNO3 ⟶ SnNO3AgCl2 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: SnCl2AgNO3 ⟶ SnNO3AgCl2 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 SnCl2AgNO3 | 1 | -1 SnNO3AgCl2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnCl2AgNO3 | 1 | -1 | ([SnCl2AgNO3])^(-1) SnNO3AgCl2 | 1 | 1 | [SnNO3AgCl2] 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 = ([SnCl2AgNO3])^(-1) [SnNO3AgCl2] = ([SnNO3AgCl2])/([SnCl2AgNO3])

Construct the rate of reaction expression for: SnCl2AgNO3 ⟶ SnNO3AgCl2 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: SnCl2AgNO3 ⟶ SnNO3AgCl2 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 SnCl2AgNO3 | 1 | -1 SnNO3AgCl2 | 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 SnCl2AgNO3 | 1 | -1 | -(Δ[SnCl2AgNO3])/(Δt) SnNO3AgCl2 | 1 | 1 | (Δ[SnNO3AgCl2])/(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[SnCl2AgNO3])/(Δt) = (Δ[SnNO3AgCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| SnCl2AgNO3 | SnNO3AgCl2 formula | SnCl2AgNO3 | SnNO3AgCl2 Hill formula | AgCl2NO3Sn | AgCl2NO3Sn

| SnCl2AgNO3 | SnNO3AgCl2 molar mass | 359.48 g/mol | 359.48 g/mol