Pb + Hg(NO3)2 = Pb(NO3)2 + Hg

Input interpretation

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Pb lead + Hg(NO_3)_2 mercury(II) nitrate ⟶ Pb(NO_3)_2 lead(II) nitrate + Hg mercury

Balanced equation

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

+ ⟶ +

Names

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lead + mercury(II) nitrate ⟶ lead(II) nitrate + mercury

Equilibrium constant

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

Rate of reaction

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