AlSn(NO3)2 = Al(NO3)2Sn

AlSn(NO3)2 ⟶ Al(NO3)2Sn

Balance the chemical equation algebraically: AlSn(NO3)2 ⟶ Al(NO3)2Sn Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AlSn(NO3)2 ⟶ c_2 Al(NO3)2Sn Set the number of atoms in the reactants equal to the number of atoms in the products for Al, Sn, N and O: Al: | c_1 = c_2 Sn: | c_1 = c_2 N: | 2 c_1 = 2 c_2 O: | 6 c_1 = 6 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: | | AlSn(NO3)2 ⟶ Al(NO3)2Sn

AlSn(NO3)2 ⟶ Al(NO3)2Sn

AlSn(NO3)2 ⟶ Al(NO3)2Sn

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

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

| AlSn(NO3)2 | Al(NO3)2Sn formula | AlSn(NO3)2 | Al(NO3)2Sn Hill formula | AlN2O6Sn | AlN2O6Sn

| AlSn(NO3)2 | Al(NO3)2Sn molar mass | 269.7 g/mol | 269.7 g/mol