Cl2 + K = KCl3

Cl_2 chlorine + K potassium ⟶ KCl3

Balance the chemical equation algebraically: Cl_2 + K ⟶ KCl3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 K ⟶ c_3 KCl3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and K: Cl: | 2 c_1 = 3 c_3 K: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 1 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Cl_2 + 2 K ⟶ 2 KCl3

+ ⟶ KCl3

chlorine + potassium ⟶ KCl3

Construct the equilibrium constant, K, expression for: Cl_2 + K ⟶ KCl3 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: 3 Cl_2 + 2 K ⟶ 2 KCl3 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 Cl_2 | 3 | -3 K | 2 | -2 KCl3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 3 | -3 | ([Cl2])^(-3) K | 2 | -2 | ([K])^(-2) KCl3 | 2 | 2 | ([KCl3])^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 = ([Cl2])^(-3) ([K])^(-2) ([KCl3])^2 = ([KCl3])^2/(([Cl2])^3 ([K])^2)

Construct the rate of reaction expression for: Cl_2 + K ⟶ KCl3 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: 3 Cl_2 + 2 K ⟶ 2 KCl3 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 Cl_2 | 3 | -3 K | 2 | -2 KCl3 | 2 | 2 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 Cl_2 | 3 | -3 | -1/3 (Δ[Cl2])/(Δt) K | 2 | -2 | -1/2 (Δ[K])/(Δt) KCl3 | 2 | 2 | 1/2 (Δ[KCl3])/(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 = -1/3 (Δ[Cl2])/(Δt) = -1/2 (Δ[K])/(Δt) = 1/2 (Δ[KCl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| chlorine | potassium | KCl3 formula | Cl_2 | K | KCl3 Hill formula | Cl_2 | K | Cl3K name | chlorine | potassium | IUPAC name | molecular chlorine | potassium |

| chlorine | potassium | KCl3 molar mass | 70.9 g/mol | 39.0983 g/mol | 145.4 g/mol phase | gas (at STP) | solid (at STP) | melting point | -101 °C | 64 °C | boiling point | -34 °C | 760 °C | density | 0.003214 g/cm^3 (at 0 °C) | 0.86 g/cm^3 | solubility in water | | reacts |