Ag + HBr = AgHBr

Ag silver + HBr hydrogen bromide ⟶ AgHBr

Balance the chemical equation algebraically: Ag + HBr ⟶ AgHBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 HBr ⟶ c_3 AgHBr Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, Br and H: Ag: | c_1 = c_3 Br: | c_2 = c_3 H: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Ag + HBr ⟶ AgHBr

+ ⟶ AgHBr

silver + hydrogen bromide ⟶ AgHBr

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

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

| silver | hydrogen bromide | AgHBr formula | Ag | HBr | AgHBr Hill formula | Ag | BrH | HAgBr name | silver | hydrogen bromide |

| silver | hydrogen bromide | AgHBr molar mass | 107.8682 g/mol | 80.912 g/mol | 188.78 g/mol phase | solid (at STP) | gas (at STP) | melting point | 960 °C | -86.8 °C | boiling point | 2212 °C | -66.38 °C | density | 10.49 g/cm^3 | 0.003307 g/cm^3 (at 25 °C) | solubility in water | insoluble | miscible | surface tension | | 0.0271 N/m | dynamic viscosity | | 8.4×10^-4 Pa s (at -75 °C) |