HNO3 + PbO = H2O + Pb(NO3)2

HNO_3 nitric acid + PbO lead monoxide ⟶ H_2O water + Pb(NO_3)_2 lead(II) nitrate

Balance the chemical equation algebraically: HNO_3 + PbO ⟶ H_2O + Pb(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 PbO ⟶ c_3 H_2O + c_4 Pb(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Pb: H: | c_1 = 2 c_3 N: | c_1 = 2 c_4 O: | 3 c_1 + c_2 = c_3 + 6 c_4 Pb: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 + PbO ⟶ H_2O + Pb(NO_3)_2

+ ⟶ +

nitric acid + lead monoxide ⟶ water + lead(II) nitrate

Construct the equilibrium constant, K, expression for: HNO_3 + PbO ⟶ H_2O + Pb(NO_3)_2 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: 2 HNO_3 + PbO ⟶ H_2O + Pb(NO_3)_2 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 HNO_3 | 2 | -2 PbO | 1 | -1 H_2O | 1 | 1 Pb(NO_3)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) PbO | 1 | -1 | ([PbO])^(-1) H_2O | 1 | 1 | [H2O] Pb(NO_3)_2 | 1 | 1 | [Pb(NO3)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 = ([HNO3])^(-2) ([PbO])^(-1) [H2O] [Pb(NO3)2] = ([H2O] [Pb(NO3)2])/(([HNO3])^2 [PbO])

Construct the rate of reaction expression for: HNO_3 + PbO ⟶ H_2O + Pb(NO_3)_2 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: 2 HNO_3 + PbO ⟶ H_2O + Pb(NO_3)_2 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 HNO_3 | 2 | -2 PbO | 1 | -1 H_2O | 1 | 1 Pb(NO_3)_2 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) PbO | 1 | -1 | -(Δ[PbO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Pb(NO_3)_2 | 1 | 1 | (Δ[Pb(NO3)2])/(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 = -1/2 (Δ[HNO3])/(Δt) = -(Δ[PbO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Pb(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | lead monoxide | water | lead(II) nitrate formula | HNO_3 | PbO | H_2O | Pb(NO_3)_2 Hill formula | HNO_3 | OPb | H_2O | N_2O_6Pb name | nitric acid | lead monoxide | water | lead(II) nitrate IUPAC name | nitric acid | | water | plumbous dinitrate

| nitric acid | lead monoxide | water | lead(II) nitrate molar mass | 63.012 g/mol | 223.2 g/mol | 18.015 g/mol | 331.2 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -41.6 °C | 886 °C | 0 °C | 470 °C boiling point | 83 °C | 1470 °C | 99.9839 °C | density | 1.5129 g/cm^3 | 9.5 g/cm^3 | 1 g/cm^3 | solubility in water | miscible | insoluble | | surface tension | | | 0.0728 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | 1.45×10^-4 Pa s (at 1000 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless | odorless