AgIHCl = AgClHI

AgIHCl ⟶ AgClHI

Balance the chemical equation algebraically: AgIHCl ⟶ AgClHI Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgIHCl ⟶ c_2 AgClHI Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, I, H and Cl: Ag: | c_1 = c_2 I: | c_1 = c_2 H: | c_1 = c_2 Cl: | c_1 = c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | AgIHCl ⟶ AgClHI

AgIHCl ⟶ AgClHI

AgIHCl ⟶ AgClHI

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

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

| AgIHCl | AgClHI formula | AgIHCl | AgClHI Hill formula | HAgClI | HAgClI

| AgIHCl | AgClHI molar mass | 271.23 g/mol | 271.23 g/mol