HCl + C3H6 = C3H7Cl

HCl hydrogen chloride + C_3H_6 cyclopropane ⟶ CH_3CH_2CH_2Cl 1-chloropropane

Balance the chemical equation algebraically: HCl + C_3H_6 ⟶ CH_3CH_2CH_2Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 C_3H_6 ⟶ c_3 CH_3CH_2CH_2Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H and C: Cl: | c_1 = c_3 H: | c_1 + 6 c_2 = 7 c_3 C: | 3 c_2 = 3 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: | | HCl + C_3H_6 ⟶ CH_3CH_2CH_2Cl

+ ⟶

hydrogen chloride + cyclopropane ⟶ 1-chloropropane

Construct the equilibrium constant, K, expression for: HCl + C_3H_6 ⟶ CH_3CH_2CH_2Cl 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: HCl + C_3H_6 ⟶ CH_3CH_2CH_2Cl 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 HCl | 1 | -1 C_3H_6 | 1 | -1 CH_3CH_2CH_2Cl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 1 | -1 | ([HCl])^(-1) C_3H_6 | 1 | -1 | ([C3H6])^(-1) CH_3CH_2CH_2Cl | 1 | 1 | [CH3CH2CH2Cl] 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 = ([HCl])^(-1) ([C3H6])^(-1) [CH3CH2CH2Cl] = ([CH3CH2CH2Cl])/([HCl] [C3H6])

Construct the rate of reaction expression for: HCl + C_3H_6 ⟶ CH_3CH_2CH_2Cl 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: HCl + C_3H_6 ⟶ CH_3CH_2CH_2Cl 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 HCl | 1 | -1 C_3H_6 | 1 | -1 CH_3CH_2CH_2Cl | 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 HCl | 1 | -1 | -(Δ[HCl])/(Δt) C_3H_6 | 1 | -1 | -(Δ[C3H6])/(Δt) CH_3CH_2CH_2Cl | 1 | 1 | (Δ[CH3CH2CH2Cl])/(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[HCl])/(Δt) = -(Δ[C3H6])/(Δt) = (Δ[CH3CH2CH2Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | cyclopropane | 1-chloropropane formula | HCl | C_3H_6 | CH_3CH_2CH_2Cl Hill formula | ClH | C_3H_6 | C_3H_7Cl name | hydrogen chloride | cyclopropane | 1-chloropropane

| hydrogen chloride | cyclopropane | 1-chloropropane molar mass | 36.46 g/mol | 42.081 g/mol | 78.54 g/mol phase | gas (at STP) | gas (at STP) | liquid (at STP) melting point | -114.17 °C | -128 °C | -123 °C boiling point | -85 °C | -33 °C | 46.5 °C density | 0.00149 g/cm^3 (at 25 °C) | 0.784 g/cm^3 (at -101 °C) | 0.892 g/cm^3 solubility in water | miscible | slightly soluble | slightly soluble surface tension | | 0.022 N/m | dynamic viscosity | | 9.303×10^-6 Pa s (at 25 °C) | 3.34×10^-4 Pa s (at 25 °C)