HCl + Ag = H2 + AgCl2

HCl hydrogen chloride + Ag silver ⟶ H_2 hydrogen + AgCl2

Balance the chemical equation algebraically: HCl + Ag ⟶ H_2 + AgCl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Ag ⟶ c_3 H_2 + c_4 AgCl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H and Ag: Cl: | c_1 = 2 c_4 H: | c_1 = 2 c_3 Ag: | 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 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + Ag ⟶ H_2 + AgCl2

+ ⟶ + AgCl2

hydrogen chloride + silver ⟶ hydrogen + AgCl2

Construct the equilibrium constant, K, expression for: HCl + Ag ⟶ H_2 + AgCl2 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 HCl + Ag ⟶ H_2 + AgCl2 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 HCl | 2 | -2 Ag | 1 | -1 H_2 | 1 | 1 AgCl2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) Ag | 1 | -1 | ([Ag])^(-1) H_2 | 1 | 1 | [H2] AgCl2 | 1 | 1 | [AgCl2] 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 = ([HCl])^(-2) ([Ag])^(-1) [H2] [AgCl2] = ([H2] [AgCl2])/(([HCl])^2 [Ag])

Construct the rate of reaction expression for: HCl + Ag ⟶ H_2 + AgCl2 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 HCl + Ag ⟶ H_2 + AgCl2 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 HCl | 2 | -2 Ag | 1 | -1 H_2 | 1 | 1 AgCl2 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) Ag | 1 | -1 | -(Δ[Ag])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) AgCl2 | 1 | 1 | (Δ[AgCl2])/(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[HCl])/(Δt) = -(Δ[Ag])/(Δt) = (Δ[H2])/(Δt) = (Δ[AgCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | silver | hydrogen | AgCl2 formula | HCl | Ag | H_2 | AgCl2 Hill formula | ClH | Ag | H_2 | AgCl2 name | hydrogen chloride | silver | hydrogen | IUPAC name | hydrogen chloride | silver | molecular hydrogen |

| hydrogen chloride | silver | hydrogen | AgCl2 molar mass | 36.46 g/mol | 107.8682 g/mol | 2.016 g/mol | 178.8 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | melting point | -114.17 °C | 960 °C | -259.2 °C | boiling point | -85 °C | 2212 °C | -252.8 °C | density | 0.00149 g/cm^3 (at 25 °C) | 10.49 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | solubility in water | miscible | insoluble | | dynamic viscosity | | | 8.9×10^-6 Pa s (at 25 °C) | odor | | | odorless |