MgCu(NO3)2 = CuMg(NO3)2

MgCu(NO3)2 ⟶ CuMg(NO3)2

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

MgCu(NO3)2 ⟶ CuMg(NO3)2

MgCu(NO3)2 ⟶ CuMg(NO3)2

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

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

| MgCu(NO3)2 | CuMg(NO3)2 formula | MgCu(NO3)2 | CuMg(NO3)2 Hill formula | CuMgN2O6 | CuMgN2O6

| MgCu(NO3)2 | CuMg(NO3)2 molar mass | 211.86 g/mol | 211.86 g/mol