Cl2 + Os = OsCl8

Cl_2 chlorine + Os osmium ⟶ OsCl8

Balance the chemical equation algebraically: Cl_2 + Os ⟶ OsCl8 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Os ⟶ c_3 OsCl8 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Os: Cl: | 2 c_1 = 8 c_3 Os: | 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 = 4 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 Cl_2 + Os ⟶ OsCl8

+ ⟶ OsCl8

chlorine + osmium ⟶ OsCl8

Construct the equilibrium constant, K, expression for: Cl_2 + Os ⟶ OsCl8 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: 4 Cl_2 + Os ⟶ OsCl8 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 | 4 | -4 Os | 1 | -1 OsCl8 | 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 | 4 | -4 | ([Cl2])^(-4) Os | 1 | -1 | ([Os])^(-1) OsCl8 | 1 | 1 | [OsCl8] 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])^(-4) ([Os])^(-1) [OsCl8] = ([OsCl8])/(([Cl2])^4 [Os])

Construct the rate of reaction expression for: Cl_2 + Os ⟶ OsCl8 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: 4 Cl_2 + Os ⟶ OsCl8 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 | 4 | -4 Os | 1 | -1 OsCl8 | 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 | 4 | -4 | -1/4 (Δ[Cl2])/(Δt) Os | 1 | -1 | -(Δ[Os])/(Δt) OsCl8 | 1 | 1 | (Δ[OsCl8])/(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 = -1/4 (Δ[Cl2])/(Δt) = -(Δ[Os])/(Δt) = (Δ[OsCl8])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| chlorine | osmium | OsCl8 formula | Cl_2 | Os | OsCl8 Hill formula | Cl_2 | Os | Cl8Os name | chlorine | osmium | IUPAC name | molecular chlorine | osmium |

| chlorine | osmium | OsCl8 molar mass | 70.9 g/mol | 190.23 g/mol | 473.8 g/mol phase | gas (at STP) | solid (at STP) | melting point | -101 °C | 3045 °C | boiling point | -34 °C | 5027 °C | density | 0.003214 g/cm^3 (at 0 °C) | 22.59 g/cm^3 | solubility in water | | insoluble |