AgNO3NaBr = AgBrNaNO3

AgNO3NaBr ⟶ AgBrNaNO3

Balance the chemical equation algebraically: AgNO3NaBr ⟶ AgBrNaNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO3NaBr ⟶ c_2 AgBrNaNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Na and Br: Ag: | c_1 = c_2 N: | c_1 = c_2 O: | 3 c_1 = 3 c_2 Na: | c_1 = c_2 Br: | 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: | | AgNO3NaBr ⟶ AgBrNaNO3

AgNO3NaBr ⟶ AgBrNaNO3

AgNO3NaBr ⟶ AgBrNaNO3

Construct the equilibrium constant, K, expression for: AgNO3NaBr ⟶ AgBrNaNO3 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: AgNO3NaBr ⟶ AgBrNaNO3 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 AgNO3NaBr | 1 | -1 AgBrNaNO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO3NaBr | 1 | -1 | ([AgNO3NaBr])^(-1) AgBrNaNO3 | 1 | 1 | [AgBrNaNO3] 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 = ([AgNO3NaBr])^(-1) [AgBrNaNO3] = ([AgBrNaNO3])/([AgNO3NaBr])

Construct the rate of reaction expression for: AgNO3NaBr ⟶ AgBrNaNO3 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: AgNO3NaBr ⟶ AgBrNaNO3 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 AgNO3NaBr | 1 | -1 AgBrNaNO3 | 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 AgNO3NaBr | 1 | -1 | -(Δ[AgNO3NaBr])/(Δt) AgBrNaNO3 | 1 | 1 | (Δ[AgBrNaNO3])/(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[AgNO3NaBr])/(Δt) = (Δ[AgBrNaNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| AgNO3NaBr | AgBrNaNO3 formula | AgNO3NaBr | AgBrNaNO3 Hill formula | AgBrNNaO3 | AgBrNNaO3

| AgNO3NaBr | AgBrNaNO3 molar mass | 272.77 g/mol | 272.77 g/mol