CaCl2 + Na = NaCl + Ca

CaCl_2 calcium chloride + Na sodium ⟶ NaCl sodium chloride + Ca calcium

Balance the chemical equation algebraically: CaCl_2 + Na ⟶ NaCl + Ca Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCl_2 + c_2 Na ⟶ c_3 NaCl + c_4 Ca Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl and Na: Ca: | c_1 = c_4 Cl: | 2 c_1 = c_3 Na: | 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CaCl_2 + 2 Na ⟶ 2 NaCl + Ca

+ ⟶ +

calcium chloride + sodium ⟶ sodium chloride + calcium

| calcium chloride | sodium | sodium chloride | calcium molecular enthalpy | -795.4 kJ/mol | 0 kJ/mol | -411.2 kJ/mol | 0 kJ/mol total enthalpy | -795.4 kJ/mol | 0 kJ/mol | -822.4 kJ/mol | 0 kJ/mol | H_initial = -795.4 kJ/mol | | H_final = -822.4 kJ/mol | ΔH_rxn^0 | -822.4 kJ/mol - -795.4 kJ/mol = -27 kJ/mol (exothermic) | | |

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

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

| calcium chloride | sodium | sodium chloride | calcium formula | CaCl_2 | Na | NaCl | Ca Hill formula | CaCl_2 | Na | ClNa | Ca name | calcium chloride | sodium | sodium chloride | calcium IUPAC name | calcium dichloride | sodium | sodium chloride | calcium