CH3OH + CH3COCl = HCl + CH3COOCH3

CH_3OH methanol + CH_3COCl acetyl chloride ⟶ HCl hydrogen chloride + CH_3COOCH_3 methyl acetate

Balance the chemical equation algebraically: CH_3OH + CH_3COCl ⟶ HCl + CH_3COOCH_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CH_3OH + c_2 CH_3COCl ⟶ c_3 HCl + c_4 CH_3COOCH_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, H, O and Cl: C: | c_1 + 2 c_2 = 3 c_4 H: | 4 c_1 + 3 c_2 = c_3 + 6 c_4 O: | c_1 + c_2 = 2 c_4 Cl: | c_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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CH_3OH + CH_3COCl ⟶ HCl + CH_3COOCH_3

+ ⟶ +

methanol + acetyl chloride ⟶ hydrogen chloride + methyl acetate

Construct the equilibrium constant, K, expression for: CH_3OH + CH_3COCl ⟶ HCl + CH_3COOCH_3 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: CH_3OH + CH_3COCl ⟶ HCl + CH_3COOCH_3 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 CH_3OH | 1 | -1 CH_3COCl | 1 | -1 HCl | 1 | 1 CH_3COOCH_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CH_3OH | 1 | -1 | ([CH3OH])^(-1) CH_3COCl | 1 | -1 | ([CH3COCl])^(-1) HCl | 1 | 1 | [HCl] CH_3COOCH_3 | 1 | 1 | [CH3COOCH3] 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 = ([CH3OH])^(-1) ([CH3COCl])^(-1) [HCl] [CH3COOCH3] = ([HCl] [CH3COOCH3])/([CH3OH] [CH3COCl])

Construct the rate of reaction expression for: CH_3OH + CH_3COCl ⟶ HCl + CH_3COOCH_3 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: CH_3OH + CH_3COCl ⟶ HCl + CH_3COOCH_3 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 CH_3OH | 1 | -1 CH_3COCl | 1 | -1 HCl | 1 | 1 CH_3COOCH_3 | 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 CH_3OH | 1 | -1 | -(Δ[CH3OH])/(Δt) CH_3COCl | 1 | -1 | -(Δ[CH3COCl])/(Δt) HCl | 1 | 1 | (Δ[HCl])/(Δt) CH_3COOCH_3 | 1 | 1 | (Δ[CH3COOCH3])/(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[CH3OH])/(Δt) = -(Δ[CH3COCl])/(Δt) = (Δ[HCl])/(Δt) = (Δ[CH3COOCH3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| methanol | acetyl chloride | hydrogen chloride | methyl acetate formula | CH_3OH | CH_3COCl | HCl | CH_3COOCH_3 Hill formula | CH_4O | C_2H_3ClO | ClH | C_3H_6O_2 name | methanol | acetyl chloride | hydrogen chloride | methyl acetate IUPAC name | methanol | acetyl chloride | hydrogen chloride | acetic acid methyl ester