Ag + KClO3 = KCl + Ag2O

Ag silver + KClO_3 potassium chlorate ⟶ KCl potassium chloride + Ag_2O silver(I) oxide

Balance the chemical equation algebraically: Ag + KClO_3 ⟶ KCl + Ag_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 KClO_3 ⟶ c_3 KCl + c_4 Ag_2O Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, Cl, K and O: Ag: | c_1 = 2 c_4 Cl: | c_2 = c_3 K: | c_2 = c_3 O: | 3 c_2 = c_4 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 = 6 c_2 = 1 c_3 = 1 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Ag + KClO_3 ⟶ KCl + 3 Ag_2O

+ ⟶ +

silver + potassium chlorate ⟶ potassium chloride + silver(I) oxide

Construct the equilibrium constant, K, expression for: Ag + KClO_3 ⟶ KCl + Ag_2O 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: 6 Ag + KClO_3 ⟶ KCl + 3 Ag_2O 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 Ag | 6 | -6 KClO_3 | 1 | -1 KCl | 1 | 1 Ag_2O | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag | 6 | -6 | ([Ag])^(-6) KClO_3 | 1 | -1 | ([KClO3])^(-1) KCl | 1 | 1 | [KCl] Ag_2O | 3 | 3 | ([Ag2O])^3 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 = ([Ag])^(-6) ([KClO3])^(-1) [KCl] ([Ag2O])^3 = ([KCl] ([Ag2O])^3)/(([Ag])^6 [KClO3])

Construct the rate of reaction expression for: Ag + KClO_3 ⟶ KCl + Ag_2O 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: 6 Ag + KClO_3 ⟶ KCl + 3 Ag_2O 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 Ag | 6 | -6 KClO_3 | 1 | -1 KCl | 1 | 1 Ag_2O | 3 | 3 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 Ag | 6 | -6 | -1/6 (Δ[Ag])/(Δt) KClO_3 | 1 | -1 | -(Δ[KClO3])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) Ag_2O | 3 | 3 | 1/3 (Δ[Ag2O])/(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 = -1/6 (Δ[Ag])/(Δt) = -(Δ[KClO3])/(Δt) = (Δ[KCl])/(Δt) = 1/3 (Δ[Ag2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver | potassium chlorate | potassium chloride | silver(I) oxide formula | Ag | KClO_3 | KCl | Ag_2O Hill formula | Ag | ClKO_3 | ClK | Ag_2O_1 name | silver | potassium chlorate | potassium chloride | silver(I) oxide

| silver | potassium chlorate | potassium chloride | silver(I) oxide molar mass | 107.8682 g/mol | 122.5 g/mol | 74.55 g/mol | 231.7 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 960 °C | 356 °C | 770 °C | boiling point | 2212 °C | | 1420 °C | density | 10.49 g/cm^3 | 2.34 g/cm^3 | 1.98 g/cm^3 | solubility in water | insoluble | soluble | soluble | odor | | | odorless |