Input interpretation
HCl (hydrogen chloride) + Fe (iron) + C_6H_5NO_2 (nitrobenzene) ⟶ H_2O (water) + FeCl_2 (iron(II) chloride) + C_6H_7N (3-methylpyridine)
Balanced equation
Balance the chemical equation algebraically: HCl + Fe + C_6H_5NO_2 ⟶ H_2O + FeCl_2 + C_6H_7N Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Fe + c_3 C_6H_5NO_2 ⟶ c_4 H_2O + c_5 FeCl_2 + c_6 C_6H_7N Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Fe, C, N and O: Cl: | c_1 = 2 c_5 H: | c_1 + 5 c_3 = 2 c_4 + 7 c_6 Fe: | c_2 = c_5 C: | 6 c_3 = 6 c_6 N: | c_3 = c_6 O: | 2 c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 3 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + 3 Fe + C_6H_5NO_2 ⟶ 2 H_2O + 3 FeCl_2 + C_6H_7N
Structures
+ + ⟶ + +
Names
hydrogen chloride + iron + nitrobenzene ⟶ water + iron(II) chloride + 3-methylpyridine
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + Fe + C_6H_5NO_2 ⟶ H_2O + FeCl_2 + C_6H_7N 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: 6 HCl + 3 Fe + C_6H_5NO_2 ⟶ 2 H_2O + 3 FeCl_2 + C_6H_7N 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 | 6 | -6 Fe | 3 | -3 C_6H_5NO_2 | 1 | -1 H_2O | 2 | 2 FeCl_2 | 3 | 3 C_6H_7N | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) Fe | 3 | -3 | ([Fe])^(-3) C_6H_5NO_2 | 1 | -1 | ([C6H5NO2])^(-1) H_2O | 2 | 2 | ([H2O])^2 FeCl_2 | 3 | 3 | ([FeCl2])^3 C_6H_7N | 1 | 1 | [C6H7N] 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])^(-6) ([Fe])^(-3) ([C6H5NO2])^(-1) ([H2O])^2 ([FeCl2])^3 [C6H7N] = (([H2O])^2 ([FeCl2])^3 [C6H7N])/(([HCl])^6 ([Fe])^3 [C6H5NO2])](../image_source/056857f92f50527a28641662263f3eb5.png)
Construct the equilibrium constant, K, expression for: HCl + Fe + C_6H_5NO_2 ⟶ H_2O + FeCl_2 + C_6H_7N 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: 6 HCl + 3 Fe + C_6H_5NO_2 ⟶ 2 H_2O + 3 FeCl_2 + C_6H_7N 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 | 6 | -6 Fe | 3 | -3 C_6H_5NO_2 | 1 | -1 H_2O | 2 | 2 FeCl_2 | 3 | 3 C_6H_7N | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) Fe | 3 | -3 | ([Fe])^(-3) C_6H_5NO_2 | 1 | -1 | ([C6H5NO2])^(-1) H_2O | 2 | 2 | ([H2O])^2 FeCl_2 | 3 | 3 | ([FeCl2])^3 C_6H_7N | 1 | 1 | [C6H7N] 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])^(-6) ([Fe])^(-3) ([C6H5NO2])^(-1) ([H2O])^2 ([FeCl2])^3 [C6H7N] = (([H2O])^2 ([FeCl2])^3 [C6H7N])/(([HCl])^6 ([Fe])^3 [C6H5NO2])
Rate of reaction
![Construct the rate of reaction expression for: HCl + Fe + C_6H_5NO_2 ⟶ H_2O + FeCl_2 + C_6H_7N 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: 6 HCl + 3 Fe + C_6H_5NO_2 ⟶ 2 H_2O + 3 FeCl_2 + C_6H_7N 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 | 6 | -6 Fe | 3 | -3 C_6H_5NO_2 | 1 | -1 H_2O | 2 | 2 FeCl_2 | 3 | 3 C_6H_7N | 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Fe | 3 | -3 | -1/3 (Δ[Fe])/(Δt) C_6H_5NO_2 | 1 | -1 | -(Δ[C6H5NO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) FeCl_2 | 3 | 3 | 1/3 (Δ[FeCl2])/(Δt) C_6H_7N | 1 | 1 | (Δ[C6H7N])/(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 = -1/6 (Δ[HCl])/(Δt) = -1/3 (Δ[Fe])/(Δt) = -(Δ[C6H5NO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[FeCl2])/(Δt) = (Δ[C6H7N])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/3c80cce8687155056bcd90724d6f58e9.png)
Construct the rate of reaction expression for: HCl + Fe + C_6H_5NO_2 ⟶ H_2O + FeCl_2 + C_6H_7N 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: 6 HCl + 3 Fe + C_6H_5NO_2 ⟶ 2 H_2O + 3 FeCl_2 + C_6H_7N 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 | 6 | -6 Fe | 3 | -3 C_6H_5NO_2 | 1 | -1 H_2O | 2 | 2 FeCl_2 | 3 | 3 C_6H_7N | 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) Fe | 3 | -3 | -1/3 (Δ[Fe])/(Δt) C_6H_5NO_2 | 1 | -1 | -(Δ[C6H5NO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) FeCl_2 | 3 | 3 | 1/3 (Δ[FeCl2])/(Δt) C_6H_7N | 1 | 1 | (Δ[C6H7N])/(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 = -1/6 (Δ[HCl])/(Δt) = -1/3 (Δ[Fe])/(Δt) = -(Δ[C6H5NO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[FeCl2])/(Δt) = (Δ[C6H7N])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| hydrogen chloride | iron | nitrobenzene | water | iron(II) chloride | 3-methylpyridine formula | HCl | Fe | C_6H_5NO_2 | H_2O | FeCl_2 | C_6H_7N Hill formula | ClH | Fe | C_6H_5NO_2 | H_2O | Cl_2Fe | C_6H_7N name | hydrogen chloride | iron | nitrobenzene | water | iron(II) chloride | 3-methylpyridine IUPAC name | hydrogen chloride | iron | nitrobenzene | water | dichloroiron | 3-methylpyridine