NaClO + NHCl2 = NaOH + NCl3

NaOCl sodium hypochlorite + NHCl2 ⟶ NaOH sodium hydroxide + N_1Cl_3 nitrogen trichloride

Balance the chemical equation algebraically: NaOCl + NHCl2 ⟶ NaOH + N_1Cl_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOCl + c_2 NHCl2 ⟶ c_3 NaOH + c_4 N_1Cl_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na, O, N and H: Cl: | c_1 + 2 c_2 = 3 c_4 Na: | c_1 = c_3 O: | c_1 = c_3 N: | c_2 = c_4 H: | c_2 = c_3 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 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaOCl + NHCl2 ⟶ NaOH + N_1Cl_3

+ NHCl2 ⟶ +

sodium hypochlorite + NHCl2 ⟶ sodium hydroxide + nitrogen trichloride

Construct the equilibrium constant, K, expression for: NaOCl + NHCl2 ⟶ NaOH + N_1Cl_3 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: NaOCl + NHCl2 ⟶ NaOH + N_1Cl_3 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 NaOCl | 1 | -1 NHCl2 | 1 | -1 NaOH | 1 | 1 N_1Cl_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOCl | 1 | -1 | ([NaOCl])^(-1) NHCl2 | 1 | -1 | ([NHCl2])^(-1) NaOH | 1 | 1 | [NaOH] N_1Cl_3 | 1 | 1 | [N1Cl3] 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 = ([NaOCl])^(-1) ([NHCl2])^(-1) [NaOH] [N1Cl3] = ([NaOH] [N1Cl3])/([NaOCl] [NHCl2])

Construct the rate of reaction expression for: NaOCl + NHCl2 ⟶ NaOH + N_1Cl_3 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: NaOCl + NHCl2 ⟶ NaOH + N_1Cl_3 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 NaOCl | 1 | -1 NHCl2 | 1 | -1 NaOH | 1 | 1 N_1Cl_3 | 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 NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) NHCl2 | 1 | -1 | -(Δ[NHCl2])/(Δt) NaOH | 1 | 1 | (Δ[NaOH])/(Δt) N_1Cl_3 | 1 | 1 | (Δ[N1Cl3])/(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[NaOCl])/(Δt) = -(Δ[NHCl2])/(Δt) = (Δ[NaOH])/(Δt) = (Δ[N1Cl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hypochlorite | NHCl2 | sodium hydroxide | nitrogen trichloride formula | NaOCl | NHCl2 | NaOH | N_1Cl_3 Hill formula | ClNaO | HCl2N | HNaO | Cl_3N name | sodium hypochlorite | | sodium hydroxide | nitrogen trichloride

| sodium hypochlorite | NHCl2 | sodium hydroxide | nitrogen trichloride molar mass | 74.44 g/mol | 85.92 g/mol | 39.997 g/mol | 120.4 g/mol phase | liquid (at STP) | | solid (at STP) | melting point | -6 °C | | 323 °C | boiling point | | | 1390 °C | density | 1.11 g/cm^3 | | 2.13 g/cm^3 | solubility in water | miscible | | soluble | surface tension | | | 0.07435 N/m | dynamic viscosity | | | 0.004 Pa s (at 350 °C) |