Ag + SO3 = Ag2SO3

Ag silver + SO_3 sulfur trioxide ⟶ Ag_2SO_3 silver(I) sulfite

Balance the chemical equation algebraically: Ag + SO_3 ⟶ Ag_2SO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 SO_3 ⟶ c_3 Ag_2SO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, O and S: Ag: | c_1 = 2 c_3 O: | 3 c_2 = 3 c_3 S: | 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 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Ag + SO_3 ⟶ Ag_2SO_3

+ ⟶

silver + sulfur trioxide ⟶ silver(I) sulfite

Construct the equilibrium constant, K, expression for: Ag + SO_3 ⟶ Ag_2SO_3 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 Ag + SO_3 ⟶ Ag_2SO_3 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 | 2 | -2 SO_3 | 1 | -1 Ag_2SO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag | 2 | -2 | ([Ag])^(-2) SO_3 | 1 | -1 | ([SO3])^(-1) Ag_2SO_3 | 1 | 1 | [Ag2SO3] 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])^(-2) ([SO3])^(-1) [Ag2SO3] = ([Ag2SO3])/(([Ag])^2 [SO3])

Construct the rate of reaction expression for: Ag + SO_3 ⟶ Ag_2SO_3 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 Ag + SO_3 ⟶ Ag_2SO_3 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 | 2 | -2 SO_3 | 1 | -1 Ag_2SO_3 | 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 Ag | 2 | -2 | -1/2 (Δ[Ag])/(Δt) SO_3 | 1 | -1 | -(Δ[SO3])/(Δt) Ag_2SO_3 | 1 | 1 | (Δ[Ag2SO3])/(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[Ag])/(Δt) = -(Δ[SO3])/(Δt) = (Δ[Ag2SO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver | sulfur trioxide | silver(I) sulfite formula | Ag | SO_3 | Ag_2SO_3 Hill formula | Ag | O_3S | Ag_2O_3S name | silver | sulfur trioxide | silver(I) sulfite IUPAC name | silver | sulfur trioxide | disilver sulfite

| silver | sulfur trioxide | silver(I) sulfite molar mass | 107.8682 g/mol | 80.06 g/mol | 295.79 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 960 °C | 16.8 °C | 100 °C boiling point | 2212 °C | 44.7 °C | density | 10.49 g/cm^3 | 1.97 g/cm^3 | solubility in water | insoluble | reacts | dynamic viscosity | | 0.00159 Pa s (at 30 °C) |