Ca(ClO)2 = CaCl2 + Ca(ClO3)2

Ca(ClO)2 ⟶ CaCl_2 calcium chloride + CaCl_2O_6 calcium chlorate

Balance the chemical equation algebraically: Ca(ClO)2 ⟶ CaCl_2 + CaCl_2O_6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(ClO)2 ⟶ c_2 CaCl_2 + c_3 CaCl_2O_6 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl and O: Ca: | c_1 = c_2 + c_3 Cl: | 2 c_1 = 2 c_2 + 2 c_3 O: | 2 c_1 = 6 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Ca(ClO)2 ⟶ 2 CaCl_2 + CaCl_2O_6

Ca(ClO)2 ⟶ +

Ca(ClO)2 ⟶ calcium chloride + calcium chlorate

Construct the equilibrium constant, K, expression for: Ca(ClO)2 ⟶ CaCl_2 + CaCl_2O_6 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 Ca(ClO)2 ⟶ 2 CaCl_2 + CaCl_2O_6 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 Ca(ClO)2 | 3 | -3 CaCl_2 | 2 | 2 CaCl_2O_6 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(ClO)2 | 3 | -3 | ([Ca(ClO)2])^(-3) CaCl_2 | 2 | 2 | ([CaCl2])^2 CaCl_2O_6 | 1 | 1 | [CaCl2O6] 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 = ([Ca(ClO)2])^(-3) ([CaCl2])^2 [CaCl2O6] = (([CaCl2])^2 [CaCl2O6])/([Ca(ClO)2])^3

Construct the rate of reaction expression for: Ca(ClO)2 ⟶ CaCl_2 + CaCl_2O_6 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 Ca(ClO)2 ⟶ 2 CaCl_2 + CaCl_2O_6 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 Ca(ClO)2 | 3 | -3 CaCl_2 | 2 | 2 CaCl_2O_6 | 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 Ca(ClO)2 | 3 | -3 | -1/3 (Δ[Ca(ClO)2])/(Δt) CaCl_2 | 2 | 2 | 1/2 (Δ[CaCl2])/(Δt) CaCl_2O_6 | 1 | 1 | (Δ[CaCl2O6])/(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[Ca(ClO)2])/(Δt) = 1/2 (Δ[CaCl2])/(Δt) = (Δ[CaCl2O6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Ca(ClO)2 | calcium chloride | calcium chlorate formula | Ca(ClO)2 | CaCl_2 | CaCl_2O_6 Hill formula | CaCl2O2 | CaCl_2 | CaCl_2O_6 name | | calcium chloride | calcium chlorate IUPAC name | | calcium dichloride | calcium dichlorate

| Ca(ClO)2 | calcium chloride | calcium chlorate molar mass | 143 g/mol | 111 g/mol | 207 g/mol phase | | solid (at STP) | solid (at STP) melting point | | 772 °C | 325 °C density | | 2.15 g/cm^3 | 2.71 g/cm^3 solubility in water | | soluble | soluble