KClO3 = O2 + KCl

KClO_3 (potassium chlorate) ⟶ O_2 (oxygen) + KCl (potassium chloride)

Balance the chemical equation algebraically: KClO_3 ⟶ O_2 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KClO_3 ⟶ c_2 O_2 + c_3 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, K and O: Cl: | c_1 = c_3 K: | c_1 = c_3 O: | 3 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 = 3/2 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KClO_3 ⟶ 3 O_2 + 2 KCl

⟶ +

potassium chlorate ⟶ oxygen + potassium chloride

| potassium chlorate | oxygen | potassium chloride molecular enthalpy | -397.7 kJ/mol | 0 kJ/mol | -436.5 kJ/mol total enthalpy | -795.4 kJ/mol | 0 kJ/mol | -873 kJ/mol | H_initial = -795.4 kJ/mol | H_final = -873 kJ/mol | ΔH_rxn^0 | -873 kJ/mol - -795.4 kJ/mol = -77.6 kJ/mol (exothermic) | |

| potassium chlorate | oxygen | potassium chloride molecular free energy | -296.3 kJ/mol | 231.7 kJ/mol | -408.5 kJ/mol total free energy | -592.6 kJ/mol | 695.1 kJ/mol | -817 kJ/mol | G_initial = -592.6 kJ/mol | G_final = -121.9 kJ/mol | ΔG_rxn^0 | -121.9 kJ/mol - -592.6 kJ/mol = 470.7 kJ/mol (endergonic) | |

| potassium chlorate | oxygen | potassium chloride molecular entropy | 143 J/(mol K) | 205 J/(mol K) | 83 J/(mol K) total entropy | 286 J/(mol K) | 615 J/(mol K) | 166 J/(mol K) | S_initial = 286 J/(mol K) | S_final = 781 J/(mol K) | ΔS_rxn^0 | 781 J/(mol K) - 286 J/(mol K) = 495 J/(mol K) (endoentropic) | |

Construct the equilibrium constant, K, expression for: KClO_3 ⟶ O_2 + KCl 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 KClO_3 ⟶ 3 O_2 + 2 KCl 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 KClO_3 | 2 | -2 O_2 | 3 | 3 KCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KClO_3 | 2 | -2 | ([KClO3])^(-2) O_2 | 3 | 3 | ([O2])^3 KCl | 2 | 2 | ([KCl])^2 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 = ([KClO3])^(-2) ([O2])^3 ([KCl])^2 = (([O2])^3 ([KCl])^2)/([KClO3])^2

Construct the rate of reaction expression for: KClO_3 ⟶ O_2 + KCl 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 KClO_3 ⟶ 3 O_2 + 2 KCl 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 KClO_3 | 2 | -2 O_2 | 3 | 3 KCl | 2 | 2 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 KClO_3 | 2 | -2 | -1/2 (Δ[KClO3])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) KCl | 2 | 2 | 1/2 (Δ[KCl])/(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[KClO3])/(Δt) = 1/3 (Δ[O2])/(Δt) = 1/2 (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium chlorate | oxygen | potassium chloride formula | KClO_3 | O_2 | KCl Hill formula | ClKO_3 | O_2 | ClK name | potassium chlorate | oxygen | potassium chloride IUPAC name | potassium chlorate | molecular oxygen | potassium chloride

| potassium chlorate | oxygen | potassium chloride molar mass | 122.5 g/mol | 31.998 g/mol | 74.55 g/mol phase | solid (at STP) | gas (at STP) | solid (at STP) melting point | 356 °C | -218 °C | 770 °C boiling point | | -183 °C | 1420 °C density | 2.34 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 1.98 g/cm^3 solubility in water | soluble | | soluble surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless