Cl2 + Ti = TiCl4

Cl_2 chlorine + Ti titanium ⟶ TiCl_4 titanium tetrachloride

Balance the chemical equation algebraically: Cl_2 + Ti ⟶ TiCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Ti ⟶ c_3 TiCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Ti: Cl: | 2 c_1 = 4 c_3 Ti: | 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 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Cl_2 + Ti ⟶ TiCl_4

+ ⟶

chlorine + titanium ⟶ titanium tetrachloride

Construct the equilibrium constant, K, expression for: Cl_2 + Ti ⟶ TiCl_4 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: 2 Cl_2 + Ti ⟶ TiCl_4 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 | 2 | -2 Ti | 1 | -1 TiCl_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 2 | -2 | ([Cl2])^(-2) Ti | 1 | -1 | ([Ti])^(-1) TiCl_4 | 1 | 1 | [TiCl4] 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])^(-2) ([Ti])^(-1) [TiCl4] = ([TiCl4])/(([Cl2])^2 [Ti])

Construct the rate of reaction expression for: Cl_2 + Ti ⟶ TiCl_4 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: 2 Cl_2 + Ti ⟶ TiCl_4 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 | 2 | -2 Ti | 1 | -1 TiCl_4 | 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 Cl_2 | 2 | -2 | -1/2 (Δ[Cl2])/(Δt) Ti | 1 | -1 | -(Δ[Ti])/(Δt) TiCl_4 | 1 | 1 | (Δ[TiCl4])/(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 = -1/2 (Δ[Cl2])/(Δt) = -(Δ[Ti])/(Δt) = (Δ[TiCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| chlorine | titanium | titanium tetrachloride formula | Cl_2 | Ti | TiCl_4 Hill formula | Cl_2 | Ti | Cl_4Ti name | chlorine | titanium | titanium tetrachloride IUPAC name | molecular chlorine | titanium | tetrachlorotitanium

| chlorine | titanium | titanium tetrachloride molar mass | 70.9 g/mol | 47.867 g/mol | 189.7 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) melting point | -101 °C | 1660 °C | -25 °C boiling point | -34 °C | 3287 °C | 135.5 °C density | 0.003214 g/cm^3 (at 0 °C) | 4.5 g/cm^3 | 1.73 g/cm^3 solubility in water | | insoluble | reacts dynamic viscosity | | | 8.27×10^-4 Pa s (at 20 °C)