Ag + HNaO3 = H2O + NaO + AgNaO3

Ag silver + HNaO3 ⟶ H_2O water + NaO + AgNaO3

Balance the chemical equation algebraically: Ag + HNaO3 ⟶ H_2O + NaO + AgNaO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 HNaO3 ⟶ c_3 H_2O + c_4 NaO + c_5 AgNaO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, H, Na and O: Ag: | c_1 = c_5 H: | c_2 = 2 c_3 Na: | c_2 = c_4 + c_5 O: | 3 c_2 = c_3 + c_4 + 3 c_5 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 4 c_3 = 2 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Ag + 4 HNaO3 ⟶ 2 H_2O + NaO + 3 AgNaO3

+ HNaO3 ⟶ + NaO + AgNaO3

silver + HNaO3 ⟶ water + NaO + AgNaO3

Construct the equilibrium constant, K, expression for: Ag + HNaO3 ⟶ H_2O + NaO + AgNaO3 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: 3 Ag + 4 HNaO3 ⟶ 2 H_2O + NaO + 3 AgNaO3 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 | 3 | -3 HNaO3 | 4 | -4 H_2O | 2 | 2 NaO | 1 | 1 AgNaO3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag | 3 | -3 | ([Ag])^(-3) HNaO3 | 4 | -4 | ([HNaO3])^(-4) H_2O | 2 | 2 | ([H2O])^2 NaO | 1 | 1 | [NaO] AgNaO3 | 3 | 3 | ([AgNaO3])^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])^(-3) ([HNaO3])^(-4) ([H2O])^2 [NaO] ([AgNaO3])^3 = (([H2O])^2 [NaO] ([AgNaO3])^3)/(([Ag])^3 ([HNaO3])^4)

Construct the rate of reaction expression for: Ag + HNaO3 ⟶ H_2O + NaO + AgNaO3 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: 3 Ag + 4 HNaO3 ⟶ 2 H_2O + NaO + 3 AgNaO3 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 | 3 | -3 HNaO3 | 4 | -4 H_2O | 2 | 2 NaO | 1 | 1 AgNaO3 | 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 | 3 | -3 | -1/3 (Δ[Ag])/(Δt) HNaO3 | 4 | -4 | -1/4 (Δ[HNaO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NaO | 1 | 1 | (Δ[NaO])/(Δt) AgNaO3 | 3 | 3 | 1/3 (Δ[AgNaO3])/(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 = -1/3 (Δ[Ag])/(Δt) = -1/4 (Δ[HNaO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NaO])/(Δt) = 1/3 (Δ[AgNaO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver | HNaO3 | water | NaO | AgNaO3 formula | Ag | HNaO3 | H_2O | NaO | AgNaO3 name | silver | | water | |

| silver | HNaO3 | water | NaO | AgNaO3 molar mass | 107.8682 g/mol | 71.995 g/mol | 18.015 g/mol | 38.989 g/mol | 178.855 g/mol phase | solid (at STP) | | liquid (at STP) | | melting point | 960 °C | | 0 °C | | boiling point | 2212 °C | | 99.9839 °C | | density | 10.49 g/cm^3 | | 1 g/cm^3 | | solubility in water | insoluble | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |