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AgNO3 + Pb = Ag + Pb(NO3)2

Input interpretation

AgNO_3 (silver nitrate) + Pb (lead) ⟶ Ag (silver) + Pb(NO_3)_2 (lead(II) nitrate)
AgNO_3 (silver nitrate) + Pb (lead) ⟶ Ag (silver) + Pb(NO_3)_2 (lead(II) nitrate)

Balanced equation

Balance the chemical equation algebraically: AgNO_3 + Pb ⟶ Ag + Pb(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 Pb ⟶ c_3 Ag + c_4 Pb(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O and Pb: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + Pb ⟶ 2 Ag + Pb(NO_3)_2
Balance the chemical equation algebraically: AgNO_3 + Pb ⟶ Ag + Pb(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 Pb ⟶ c_3 Ag + c_4 Pb(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O and Pb: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + Pb ⟶ 2 Ag + Pb(NO_3)_2

Structures

+ ⟶ +
+ ⟶ +

Names

silver nitrate + lead ⟶ silver + lead(II) nitrate
silver nitrate + lead ⟶ silver + lead(II) nitrate

Reaction thermodynamics

Enthalpy

| silver nitrate | lead | silver | lead(II) nitrate molecular enthalpy | -124.4 kJ/mol | 0 kJ/mol | 0 kJ/mol | -451.9 kJ/mol total enthalpy | -248.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | -451.9 kJ/mol | H_initial = -248.8 kJ/mol | | H_final = -451.9 kJ/mol | ΔH_rxn^0 | -451.9 kJ/mol - -248.8 kJ/mol = -203.1 kJ/mol (exothermic) | | |
| silver nitrate | lead | silver | lead(II) nitrate molecular enthalpy | -124.4 kJ/mol | 0 kJ/mol | 0 kJ/mol | -451.9 kJ/mol total enthalpy | -248.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | -451.9 kJ/mol | H_initial = -248.8 kJ/mol | | H_final = -451.9 kJ/mol | ΔH_rxn^0 | -451.9 kJ/mol - -248.8 kJ/mol = -203.1 kJ/mol (exothermic) | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: AgNO_3 + Pb ⟶ Ag + 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 AgNO_3 + Pb ⟶ 2 Ag + 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 AgNO_3 | 2 | -2 Pb | 1 | -1 Ag | 2 | 2 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 AgNO_3 | 2 | -2 | ([AgNO3])^(-2) Pb | 1 | -1 | ([Pb])^(-1) Ag | 2 | 2 | ([Ag])^2 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 = ([AgNO3])^(-2) ([Pb])^(-1) ([Ag])^2 [Pb(NO3)2] = (([Ag])^2 [Pb(NO3)2])/(([AgNO3])^2 [Pb])
Construct the equilibrium constant, K, expression for: AgNO_3 + Pb ⟶ Ag + 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 AgNO_3 + Pb ⟶ 2 Ag + 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 AgNO_3 | 2 | -2 Pb | 1 | -1 Ag | 2 | 2 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 AgNO_3 | 2 | -2 | ([AgNO3])^(-2) Pb | 1 | -1 | ([Pb])^(-1) Ag | 2 | 2 | ([Ag])^2 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 = ([AgNO3])^(-2) ([Pb])^(-1) ([Ag])^2 [Pb(NO3)2] = (([Ag])^2 [Pb(NO3)2])/(([AgNO3])^2 [Pb])

Rate of reaction

Construct the rate of reaction expression for: AgNO_3 + Pb ⟶ Ag + 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 AgNO_3 + Pb ⟶ 2 Ag + 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 AgNO_3 | 2 | -2 Pb | 1 | -1 Ag | 2 | 2 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 AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) Pb | 1 | -1 | -(Δ[Pb])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(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[AgNO3])/(Δt) = -(Δ[Pb])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[Pb(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: AgNO_3 + Pb ⟶ Ag + 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 AgNO_3 + Pb ⟶ 2 Ag + 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 AgNO_3 | 2 | -2 Pb | 1 | -1 Ag | 2 | 2 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 AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) Pb | 1 | -1 | -(Δ[Pb])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(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[AgNO3])/(Δt) = -(Δ[Pb])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[Pb(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| silver nitrate | lead | silver | lead(II) nitrate formula | AgNO_3 | Pb | Ag | Pb(NO_3)_2 Hill formula | AgNO_3 | Pb | Ag | N_2O_6Pb name | silver nitrate | lead | silver | lead(II) nitrate IUPAC name | silver nitrate | lead | silver | plumbous dinitrate
| silver nitrate | lead | silver | lead(II) nitrate formula | AgNO_3 | Pb | Ag | Pb(NO_3)_2 Hill formula | AgNO_3 | Pb | Ag | N_2O_6Pb name | silver nitrate | lead | silver | lead(II) nitrate IUPAC name | silver nitrate | lead | silver | plumbous dinitrate

Substance properties

| silver nitrate | lead | silver | lead(II) nitrate molar mass | 169.87 g/mol | 207.2 g/mol | 107.8682 g/mol | 331.2 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 327.4 °C | 960 °C | 470 °C boiling point | | 1740 °C | 2212 °C | density | | 11.34 g/cm^3 | 10.49 g/cm^3 | solubility in water | soluble | insoluble | insoluble | dynamic viscosity | | 0.00183 Pa s (at 38 °C) | | odor | odorless | | | odorless
| silver nitrate | lead | silver | lead(II) nitrate molar mass | 169.87 g/mol | 207.2 g/mol | 107.8682 g/mol | 331.2 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 327.4 °C | 960 °C | 470 °C boiling point | | 1740 °C | 2212 °C | density | | 11.34 g/cm^3 | 10.49 g/cm^3 | solubility in water | soluble | insoluble | insoluble | dynamic viscosity | | 0.00183 Pa s (at 38 °C) | | odor | odorless | | | odorless

Units

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