CH3COONH4 = H2O + CH3C(O)NH2

CH_3CO_2NH_4 ammonium acetate ⟶ H_2O water + CH_3CONH_2 acetamide

Balance the chemical equation algebraically: CH_3CO_2NH_4 ⟶ H_2O + CH_3CONH_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CH_3CO_2NH_4 ⟶ c_2 H_2O + c_3 CH_3CONH_2 Set the number of atoms in the reactants equal to the number of atoms in the products for C, H, N and O: C: | 2 c_1 = 2 c_3 H: | 7 c_1 = 2 c_2 + 5 c_3 N: | c_1 = c_3 O: | 2 c_1 = 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CH_3CO_2NH_4 ⟶ H_2O + CH_3CONH_2

⟶ +

ammonium acetate ⟶ water + acetamide

Construct the equilibrium constant, K, expression for: CH_3CO_2NH_4 ⟶ H_2O + CH_3CONH_2 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_3CO_2NH_4 ⟶ H_2O + CH_3CONH_2 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_3CO_2NH_4 | 1 | -1 H_2O | 1 | 1 CH_3CONH_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CH_3CO_2NH_4 | 1 | -1 | ([CH3CO2NH4])^(-1) H_2O | 1 | 1 | [H2O] CH_3CONH_2 | 1 | 1 | [CH3CONH2] 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 = ([CH3CO2NH4])^(-1) [H2O] [CH3CONH2] = ([H2O] [CH3CONH2])/([CH3CO2NH4])

Construct the rate of reaction expression for: CH_3CO_2NH_4 ⟶ H_2O + CH_3CONH_2 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_3CO_2NH_4 ⟶ H_2O + CH_3CONH_2 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_3CO_2NH_4 | 1 | -1 H_2O | 1 | 1 CH_3CONH_2 | 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_3CO_2NH_4 | 1 | -1 | -(Δ[CH3CO2NH4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CH_3CONH_2 | 1 | 1 | (Δ[CH3CONH2])/(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[CH3CO2NH4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CH3CONH2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| ammonium acetate | water | acetamide formula | CH_3CO_2NH_4 | H_2O | CH_3CONH_2 Hill formula | C_2H_7NO_2 | H_2O | C_2H_5NO name | ammonium acetate | water | acetamide

| ammonium acetate | water | acetamide molar mass | 77.08 g/mol | 18.015 g/mol | 59.07 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 111 °C | 0 °C | 79 °C boiling point | | 99.9839 °C | 221 °C density | 1.171 g/cm^3 | 1 g/cm^3 | 1.14 g/cm^3 solubility in water | slightly soluble | | surface tension | | 0.0728 N/m | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | 0.00132 Pa s (at 105 °C) odor | | odorless |