H2 + AgNO2 = H2O + NO + Ag

H_2 hydrogen + AgNO_2 silver nitrite ⟶ H_2O water + NO nitric oxide + Ag silver

Balance the chemical equation algebraically: H_2 + AgNO_2 ⟶ H_2O + NO + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 AgNO_2 ⟶ c_3 H_2O + c_4 NO + c_5 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, Ag, N and O: H: | 2 c_1 = 2 c_3 Ag: | c_2 = c_5 N: | c_2 = c_4 O: | 2 c_2 = c_3 + 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + AgNO_2 ⟶ H_2O + NO + Ag

+ ⟶ + +

hydrogen + silver nitrite ⟶ water + nitric oxide + silver

Construct the equilibrium constant, K, expression for: H_2 + AgNO_2 ⟶ H_2O + NO + Ag 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: H_2 + AgNO_2 ⟶ H_2O + NO + Ag 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 H_2 | 1 | -1 AgNO_2 | 1 | -1 H_2O | 1 | 1 NO | 1 | 1 Ag | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2 | 1 | -1 | ([H2])^(-1) AgNO_2 | 1 | -1 | ([AgNO2])^(-1) H_2O | 1 | 1 | [H2O] NO | 1 | 1 | [NO] Ag | 1 | 1 | [Ag] 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 = ([H2])^(-1) ([AgNO2])^(-1) [H2O] [NO] [Ag] = ([H2O] [NO] [Ag])/([H2] [AgNO2])

Construct the rate of reaction expression for: H_2 + AgNO_2 ⟶ H_2O + NO + Ag 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: H_2 + AgNO_2 ⟶ H_2O + NO + Ag 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 H_2 | 1 | -1 AgNO_2 | 1 | -1 H_2O | 1 | 1 NO | 1 | 1 Ag | 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 H_2 | 1 | -1 | -(Δ[H2])/(Δt) AgNO_2 | 1 | -1 | -(Δ[AgNO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) Ag | 1 | 1 | (Δ[Ag])/(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[H2])/(Δt) = -(Δ[AgNO2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen | silver nitrite | water | nitric oxide | silver formula | H_2 | AgNO_2 | H_2O | NO | Ag name | hydrogen | silver nitrite | water | nitric oxide | silver IUPAC name | molecular hydrogen | silver nitrite | water | nitric oxide | silver