H2SO4 + Zn + AgCl = HCl + Ag + ZnSO4

Input interpretation

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H_2SO_4 sulfuric acid + Zn zinc + AgCl silver chloride ⟶ HCl hydrogen chloride + Ag silver + ZnSO_4 zinc sulfate

Balanced equation

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Balance the chemical equation algebraically: H_2SO_4 + Zn + AgCl ⟶ HCl + Ag + ZnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Zn + c_3 AgCl ⟶ c_4 HCl + c_5 Ag + c_6 ZnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Zn, Ag and Cl: H: | 2 c_1 = c_4 O: | 4 c_1 = 4 c_6 S: | c_1 = c_6 Zn: | c_2 = c_6 Ag: | c_3 = c_5 Cl: | 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 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + Zn + 2 AgCl ⟶ 2 HCl + 2 Ag + ZnSO_4

+ + ⟶ + +

Names

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sulfuric acid + zinc + silver chloride ⟶ hydrogen chloride + silver + zinc sulfate

Equilibrium constant

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Construct the equilibrium constant, K, expression for: H_2SO_4 + Zn + AgCl ⟶ HCl + Ag + ZnSO_4 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_2SO_4 + Zn + 2 AgCl ⟶ 2 HCl + 2 Ag + ZnSO_4 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_2SO_4 | 1 | -1 Zn | 1 | -1 AgCl | 2 | -2 HCl | 2 | 2 Ag | 2 | 2 ZnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) Zn | 1 | -1 | ([Zn])^(-1) AgCl | 2 | -2 | ([AgCl])^(-2) HCl | 2 | 2 | ([HCl])^2 Ag | 2 | 2 | ([Ag])^2 ZnSO_4 | 1 | 1 | [ZnSO4] 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 = ([H2SO4])^(-1) ([Zn])^(-1) ([AgCl])^(-2) ([HCl])^2 ([Ag])^2 [ZnSO4] = (([HCl])^2 ([Ag])^2 [ZnSO4])/([H2SO4] [Zn] ([AgCl])^2)

Rate of reaction

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Construct the rate of reaction expression for: H_2SO_4 + Zn + AgCl ⟶ HCl + Ag + ZnSO_4 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_2SO_4 + Zn + 2 AgCl ⟶ 2 HCl + 2 Ag + ZnSO_4 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_2SO_4 | 1 | -1 Zn | 1 | -1 AgCl | 2 | -2 HCl | 2 | 2 Ag | 2 | 2 ZnSO_4 | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) Zn | 1 | -1 | -(Δ[Zn])/(Δt) AgCl | 2 | -2 | -1/2 (Δ[AgCl])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(Δt) ZnSO_4 | 1 | 1 | (Δ[ZnSO4])/(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[H2SO4])/(Δt) = -(Δ[Zn])/(Δt) = -1/2 (Δ[AgCl])/(Δt) = 1/2 (Δ[HCl])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[ZnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)