Ni(ClO3)2 = O2 + NiCl2

Ni(ClO3)2 ⟶ O_2 oxygen + NiCl_2 nickel(II) chloride

Balance the chemical equation algebraically: Ni(ClO3)2 ⟶ O_2 + NiCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ni(ClO3)2 ⟶ c_2 O_2 + c_3 NiCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ni, Cl and O: Ni: | c_1 = c_3 Cl: | 2 c_1 = 2 c_3 O: | 6 c_1 = 2 c_2 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 = 3 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Ni(ClO3)2 ⟶ 3 O_2 + NiCl_2

Ni(ClO3)2 ⟶ +

Ni(ClO3)2 ⟶ oxygen + nickel(II) chloride

Construct the equilibrium constant, K, expression for: Ni(ClO3)2 ⟶ O_2 + NiCl_2 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: Ni(ClO3)2 ⟶ 3 O_2 + NiCl_2 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 Ni(ClO3)2 | 1 | -1 O_2 | 3 | 3 NiCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ni(ClO3)2 | 1 | -1 | ([Ni(ClO3)2])^(-1) O_2 | 3 | 3 | ([O2])^3 NiCl_2 | 1 | 1 | [NiCl2] 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 = ([Ni(ClO3)2])^(-1) ([O2])^3 [NiCl2] = (([O2])^3 [NiCl2])/([Ni(ClO3)2])

Construct the rate of reaction expression for: Ni(ClO3)2 ⟶ O_2 + NiCl_2 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: Ni(ClO3)2 ⟶ 3 O_2 + NiCl_2 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 Ni(ClO3)2 | 1 | -1 O_2 | 3 | 3 NiCl_2 | 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 Ni(ClO3)2 | 1 | -1 | -(Δ[Ni(ClO3)2])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) NiCl_2 | 1 | 1 | (Δ[NiCl2])/(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[Ni(ClO3)2])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[NiCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| Ni(ClO3)2 | oxygen | nickel(II) chloride formula | Ni(ClO3)2 | O_2 | NiCl_2 Hill formula | Cl2NiO6 | O_2 | Cl_2Ni name | | oxygen | nickel(II) chloride IUPAC name | | molecular oxygen | dichloronickel

| Ni(ClO3)2 | oxygen | nickel(II) chloride molar mass | 225.6 g/mol | 31.998 g/mol | 129.6 g/mol phase | | gas (at STP) | melting point | | -218 °C | boiling point | | -183 °C | density | | 0.001429 g/cm^3 (at 0 °C) | 3.55 g/cm^3 surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless |