NH4ClNaOH = NH3H2ONaCl

NH4ClNaOH ⟶ NH3H2ONaCl

Balance the chemical equation algebraically: NH4ClNaOH ⟶ NH3H2ONaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH4ClNaOH ⟶ c_2 NH3H2ONaCl Set the number of atoms in the reactants equal to the number of atoms in the products for N, H, Cl, Na and O: N: | c_1 = c_2 H: | 5 c_1 = 5 c_2 Cl: | c_1 = c_2 Na: | c_1 = c_2 O: | c_1 = 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: | | NH4ClNaOH ⟶ NH3H2ONaCl

NH4ClNaOH ⟶ NH3H2ONaCl

NH4ClNaOH ⟶ NH3H2ONaCl

Construct the equilibrium constant, K, expression for: NH4ClNaOH ⟶ NH3H2ONaCl 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: NH4ClNaOH ⟶ NH3H2ONaCl 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 NH4ClNaOH | 1 | -1 NH3H2ONaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH4ClNaOH | 1 | -1 | ([NH4ClNaOH])^(-1) NH3H2ONaCl | 1 | 1 | [NH3H2ONaCl] 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 = ([NH4ClNaOH])^(-1) [NH3H2ONaCl] = ([NH3H2ONaCl])/([NH4ClNaOH])

Construct the rate of reaction expression for: NH4ClNaOH ⟶ NH3H2ONaCl 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: NH4ClNaOH ⟶ NH3H2ONaCl 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 NH4ClNaOH | 1 | -1 NH3H2ONaCl | 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 NH4ClNaOH | 1 | -1 | -(Δ[NH4ClNaOH])/(Δt) NH3H2ONaCl | 1 | 1 | (Δ[NH3H2ONaCl])/(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[NH4ClNaOH])/(Δt) = (Δ[NH3H2ONaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| NH4ClNaOH | NH3H2ONaCl formula | NH4ClNaOH | NH3H2ONaCl Hill formula | H5ClNNaO | H5ClNNaO

| NH4ClNaOH | NH3H2ONaCl molar mass | 93.49 g/mol | 93.49 g/mol