NaClNH4HCO3 = NaHCO3NH4Cl

NaClNH4HCO3 ⟶ NaHCO3NH4Cl

Balance the chemical equation algebraically: NaClNH4HCO3 ⟶ NaHCO3NH4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaClNH4HCO3 ⟶ c_2 NaHCO3NH4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Na, Cl, N, H, C and O: Na: | c_1 = c_2 Cl: | c_1 = c_2 N: | c_1 = c_2 H: | 5 c_1 = 5 c_2 C: | 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: | | NaClNH4HCO3 ⟶ NaHCO3NH4Cl

NaClNH4HCO3 ⟶ NaHCO3NH4Cl

NaClNH4HCO3 ⟶ NaHCO3NH4Cl

Construct the equilibrium constant, K, expression for: NaClNH4HCO3 ⟶ NaHCO3NH4Cl 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: NaClNH4HCO3 ⟶ NaHCO3NH4Cl 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 NaClNH4HCO3 | 1 | -1 NaHCO3NH4Cl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaClNH4HCO3 | 1 | -1 | ([NaClNH4HCO3])^(-1) NaHCO3NH4Cl | 1 | 1 | [NaHCO3NH4Cl] 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 = ([NaClNH4HCO3])^(-1) [NaHCO3NH4Cl] = ([NaHCO3NH4Cl])/([NaClNH4HCO3])

Construct the rate of reaction expression for: NaClNH4HCO3 ⟶ NaHCO3NH4Cl 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: NaClNH4HCO3 ⟶ NaHCO3NH4Cl 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 NaClNH4HCO3 | 1 | -1 NaHCO3NH4Cl | 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 NaClNH4HCO3 | 1 | -1 | -(Δ[NaClNH4HCO3])/(Δt) NaHCO3NH4Cl | 1 | 1 | (Δ[NaHCO3NH4Cl])/(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[NaClNH4HCO3])/(Δt) = (Δ[NaHCO3NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| NaClNH4HCO3 | NaHCO3NH4Cl formula | NaClNH4HCO3 | NaHCO3NH4Cl Hill formula | CH5ClNNaO3 | CH5ClNNaO3

| NaClNH4HCO3 | NaHCO3NH4Cl molar mass | 137.5 g/mol | 137.5 g/mol