Cl2 + Pt = PtCl4

Cl_2 chlorine + Pt platinum ⟶ PtCl_4 platinum(IV) chloride

Balance the chemical equation algebraically: Cl_2 + Pt ⟶ PtCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Pt ⟶ c_3 PtCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Pt: Cl: | 2 c_1 = 4 c_3 Pt: | 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 + Pt ⟶ PtCl_4

+ ⟶

chlorine + platinum ⟶ platinum(IV) chloride

| chlorine | platinum | platinum(IV) chloride molecular enthalpy | 0 kJ/mol | 0 kJ/mol | -231.8 kJ/mol total enthalpy | 0 kJ/mol | 0 kJ/mol | -231.8 kJ/mol | H_initial = 0 kJ/mol | | H_final = -231.8 kJ/mol ΔH_rxn^0 | -231.8 kJ/mol - 0 kJ/mol = -231.8 kJ/mol (exothermic) | |

Construct the equilibrium constant, K, expression for: Cl_2 + Pt ⟶ PtCl_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 + Pt ⟶ PtCl_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 Pt | 1 | -1 PtCl_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) Pt | 1 | -1 | ([Pt])^(-1) PtCl_4 | 1 | 1 | [PtCl4] 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) ([Pt])^(-1) [PtCl4] = ([PtCl4])/(([Cl2])^2 [Pt])

Construct the rate of reaction expression for: Cl_2 + Pt ⟶ PtCl_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 + Pt ⟶ PtCl_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 Pt | 1 | -1 PtCl_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) Pt | 1 | -1 | -(Δ[Pt])/(Δt) PtCl_4 | 1 | 1 | (Δ[PtCl4])/(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[Pt])/(Δt) = (Δ[PtCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| chlorine | platinum | platinum(IV) chloride formula | Cl_2 | Pt | PtCl_4 Hill formula | Cl_2 | Pt | Cl_4Pt name | chlorine | platinum | platinum(IV) chloride IUPAC name | molecular chlorine | platinum | tetrachloroplatinum

| chlorine | platinum | platinum(IV) chloride molar mass | 70.9 g/mol | 195.084 g/mol | 336.9 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) melting point | -101 °C | 1772 °C | 370 °C boiling point | -34 °C | 3827 °C | density | 0.003214 g/cm^3 (at 0 °C) | 21.45 g/cm^3 | 4.303 g/cm^3 solubility in water | | insoluble |