H2 + Ag2O = H2O + Ag

H_2 hydrogen + Ag_2O silver(I) oxide ⟶ H_2O water + Ag silver

Balance the chemical equation algebraically: H_2 + Ag_2O ⟶ H_2O + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 Ag_2O ⟶ c_3 H_2O + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Ag: H: | 2 c_1 = 2 c_3 O: | c_2 = c_3 Ag: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + Ag_2O ⟶ H_2O + 2 Ag

+ ⟶ +

hydrogen + silver(I) oxide ⟶ water + silver

Construct the equilibrium constant, K, expression for: H_2 + Ag_2O ⟶ H_2O + 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 + Ag_2O ⟶ H_2O + 2 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 Ag_2O | 1 | -1 H_2O | 1 | 1 Ag | 2 | 2 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) Ag_2O | 1 | -1 | ([Ag2O])^(-1) H_2O | 1 | 1 | [H2O] Ag | 2 | 2 | ([Ag])^2 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) ([Ag2O])^(-1) [H2O] ([Ag])^2 = ([H2O] ([Ag])^2)/([H2] [Ag2O])

Construct the rate of reaction expression for: H_2 + Ag_2O ⟶ H_2O + 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 + Ag_2O ⟶ H_2O + 2 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 Ag_2O | 1 | -1 H_2O | 1 | 1 Ag | 2 | 2 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) Ag_2O | 1 | -1 | -(Δ[Ag2O])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Ag | 2 | 2 | 1/2 (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[Ag2O])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen | silver(I) oxide | water | silver formula | H_2 | Ag_2O | H_2O | Ag Hill formula | H_2 | Ag_2O_1 | H_2O | Ag name | hydrogen | silver(I) oxide | water | silver IUPAC name | molecular hydrogen | | water | silver

| hydrogen | silver(I) oxide | water | silver molar mass | 2.016 g/mol | 231.7 g/mol | 18.015 g/mol | 107.8682 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | -259.2 °C | | 0 °C | 960 °C boiling point | -252.8 °C | | 99.9839 °C | 2212 °C density | 8.99×10^-5 g/cm^3 (at 0 °C) | | 1 g/cm^3 | 10.49 g/cm^3 solubility in water | | | | insoluble surface tension | | | 0.0728 N/m | dynamic viscosity | 8.9×10^-6 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |