FeSO4 + SnSO4 = Fe2(SO4)3 + Sn

Input interpretation

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FeSO_4 duretter + SnSO_4 stannous sulfate ⟶ Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + Sn white tin

Balanced equation

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Balance the chemical equation algebraically: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO_4 + c_2 SnSO_4 ⟶ c_3 Fe_2(SO_4)_3·xH_2O + c_4 Sn Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S and Sn: Fe: | c_1 = 2 c_3 O: | 4 c_1 + 4 c_2 = 12 c_3 S: | c_1 + c_2 = 3 c_3 Sn: | 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 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn

+ ⟶ +

Names

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duretter + stannous sulfate ⟶ iron(III) sulfate hydrate + white tin

Equilibrium constant

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Construct the equilibrium constant, K, expression for: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 | 2 | -2 SnSO_4 | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Sn | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeSO_4 | 2 | -2 | ([FeSO4])^(-2) SnSO_4 | 1 | -1 | ([SnSO4])^(-1) Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] Sn | 1 | 1 | [Sn] 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 = ([FeSO4])^(-2) ([SnSO4])^(-1) [Fe2(SO4)3·xH2O] [Sn] = ([Fe2(SO4)3·xH2O] [Sn])/(([FeSO4])^2 [SnSO4])

Rate of reaction

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Construct the rate of reaction expression for: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 | 2 | -2 SnSO_4 | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Sn | 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 FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) SnSO_4 | 1 | -1 | -(Δ[SnSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(Δt) Sn | 1 | 1 | (Δ[Sn])/(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[FeSO4])/(Δt) = -(Δ[SnSO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) = (Δ[Sn])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)