NaCl + KNO3 = KClNaNO3

NaCl sodium chloride + KNO_3 potassium nitrate ⟶ KClNaNO3

Balance the chemical equation algebraically: NaCl + KNO_3 ⟶ KClNaNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaCl + c_2 KNO_3 ⟶ c_3 KClNaNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na, K, N and O: Cl: | c_1 = c_3 Na: | c_1 = c_3 K: | c_2 = c_3 N: | c_2 = c_3 O: | 3 c_2 = 3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaCl + KNO_3 ⟶ KClNaNO3

+ ⟶ KClNaNO3

sodium chloride + potassium nitrate ⟶ KClNaNO3

Construct the equilibrium constant, K, expression for: NaCl + KNO_3 ⟶ KClNaNO3 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: NaCl + KNO_3 ⟶ KClNaNO3 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 NaCl | 1 | -1 KNO_3 | 1 | -1 KClNaNO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaCl | 1 | -1 | ([NaCl])^(-1) KNO_3 | 1 | -1 | ([KNO3])^(-1) KClNaNO3 | 1 | 1 | [KClNaNO3] 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 = ([NaCl])^(-1) ([KNO3])^(-1) [KClNaNO3] = ([KClNaNO3])/([NaCl] [KNO3])

Construct the rate of reaction expression for: NaCl + KNO_3 ⟶ KClNaNO3 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: NaCl + KNO_3 ⟶ KClNaNO3 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 NaCl | 1 | -1 KNO_3 | 1 | -1 KClNaNO3 | 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 NaCl | 1 | -1 | -(Δ[NaCl])/(Δt) KNO_3 | 1 | -1 | -(Δ[KNO3])/(Δt) KClNaNO3 | 1 | 1 | (Δ[KClNaNO3])/(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[NaCl])/(Δt) = -(Δ[KNO3])/(Δt) = (Δ[KClNaNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium chloride | potassium nitrate | KClNaNO3 formula | NaCl | KNO_3 | KClNaNO3 Hill formula | ClNa | KNO_3 | ClKNNaO3 name | sodium chloride | potassium nitrate |

| sodium chloride | potassium nitrate | KClNaNO3 molar mass | 58.44 g/mol | 101.1 g/mol | 159.54 g/mol phase | solid (at STP) | solid (at STP) | melting point | 801 °C | 334 °C | boiling point | 1413 °C | | density | 2.16 g/cm^3 | | solubility in water | soluble | soluble | odor | odorless | odorless |