H2SO4 + Ca(CH3COO)2 = CH3COOH + CaSO4

Input interpretation

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H_2SO_4 sulfuric acid + Ca(CH3COO)2 ⟶ CH_3CO_2H acetic acid + CaSO_4 calcium sulfate

Balanced equation

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Balance the chemical equation algebraically: H_2SO_4 + Ca(CH3COO)2 ⟶ CH_3CO_2H + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Ca(CH3COO)2 ⟶ c_3 CH_3CO_2H + c_4 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Ca and C: H: | 2 c_1 + 6 c_2 = 4 c_3 O: | 4 c_1 + 4 c_2 = 2 c_3 + 4 c_4 S: | c_1 = c_4 Ca: | c_2 = c_4 C: | 4 c_2 = 2 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + Ca(CH3COO)2 ⟶ 2 CH_3CO_2H + CaSO_4

+ Ca(CH3COO)2 ⟶ +

Names

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sulfuric acid + Ca(CH3COO)2 ⟶ acetic acid + calcium sulfate

Equilibrium constant

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Construct the equilibrium constant, K, expression for: H_2SO_4 + Ca(CH3COO)2 ⟶ CH_3CO_2H + CaSO_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 + Ca(CH3COO)2 ⟶ 2 CH_3CO_2H + CaSO_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 Ca(CH3COO)2 | 1 | -1 CH_3CO_2H | 2 | 2 CaSO_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) Ca(CH3COO)2 | 1 | -1 | ([Ca(CH3COO)2])^(-1) CH_3CO_2H | 2 | 2 | ([CH3CO2H])^2 CaSO_4 | 1 | 1 | [CaSO4] 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) ([Ca(CH3COO)2])^(-1) ([CH3CO2H])^2 [CaSO4] = (([CH3CO2H])^2 [CaSO4])/([H2SO4] [Ca(CH3COO)2])

Rate of reaction

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Construct the rate of reaction expression for: H_2SO_4 + Ca(CH3COO)2 ⟶ CH_3CO_2H + CaSO_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 + Ca(CH3COO)2 ⟶ 2 CH_3CO_2H + CaSO_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 Ca(CH3COO)2 | 1 | -1 CH_3CO_2H | 2 | 2 CaSO_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) Ca(CH3COO)2 | 1 | -1 | -(Δ[Ca(CH3COO)2])/(Δt) CH_3CO_2H | 2 | 2 | 1/2 (Δ[CH3CO2H])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[Ca(CH3COO)2])/(Δt) = 1/2 (Δ[CH3CO2H])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)