Input interpretation
![H_2O (water) + Cl_2 (chlorine) ⟶ HCl (hydrogen chloride) + HOCl (hypochlorous acid)](../image_source/84014b8cef92e7744aa9430dcc577ebd.png)
H_2O (water) + Cl_2 (chlorine) ⟶ HCl (hydrogen chloride) + HOCl (hypochlorous acid)
Balanced equation
![Balance the chemical equation algebraically: H_2O + Cl_2 ⟶ HCl + HOCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 ⟶ c_3 HCl + c_4 HOCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Cl: H: | 2 c_1 = c_3 + c_4 O: | c_1 = c_4 Cl: | 2 c_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_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: | | H_2O + Cl_2 ⟶ HCl + HOCl](../image_source/723b8bc9dc2a5ef0ad30222149b81f41.png)
Balance the chemical equation algebraically: H_2O + Cl_2 ⟶ HCl + HOCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 ⟶ c_3 HCl + c_4 HOCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Cl: H: | 2 c_1 = c_3 + c_4 O: | c_1 = c_4 Cl: | 2 c_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_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: | | H_2O + Cl_2 ⟶ HCl + HOCl
Structures
![+ ⟶ +](../image_source/793496b91c3b050903ea1b9ee855a121.png)
+ ⟶ +
Names
![water + chlorine ⟶ hydrogen chloride + hypochlorous acid](../image_source/6288f5a901e8fd405fc37053ff4e92e6.png)
water + chlorine ⟶ hydrogen chloride + hypochlorous acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2O + Cl_2 ⟶ HCl + HOCl 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_2O + Cl_2 ⟶ HCl + HOCl 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_2O | 1 | -1 Cl_2 | 1 | -1 HCl | 1 | 1 HOCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) Cl_2 | 1 | -1 | ([Cl2])^(-1) HCl | 1 | 1 | [HCl] HOCl | 1 | 1 | [HOCl] 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 = ([H2O])^(-1) ([Cl2])^(-1) [HCl] [HOCl] = ([HCl] [HOCl])/([H2O] [Cl2])](../image_source/42c4888f6375691c98b438c2d1029030.png)
Construct the equilibrium constant, K, expression for: H_2O + Cl_2 ⟶ HCl + HOCl 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_2O + Cl_2 ⟶ HCl + HOCl 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_2O | 1 | -1 Cl_2 | 1 | -1 HCl | 1 | 1 HOCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) Cl_2 | 1 | -1 | ([Cl2])^(-1) HCl | 1 | 1 | [HCl] HOCl | 1 | 1 | [HOCl] 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 = ([H2O])^(-1) ([Cl2])^(-1) [HCl] [HOCl] = ([HCl] [HOCl])/([H2O] [Cl2])
Rate of reaction
![Construct the rate of reaction expression for: H_2O + Cl_2 ⟶ HCl + HOCl 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_2O + Cl_2 ⟶ HCl + HOCl 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_2O | 1 | -1 Cl_2 | 1 | -1 HCl | 1 | 1 HOCl | 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_2O | 1 | -1 | -(Δ[H2O])/(Δt) Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) HCl | 1 | 1 | (Δ[HCl])/(Δt) HOCl | 1 | 1 | (Δ[HOCl])/(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[H2O])/(Δt) = -(Δ[Cl2])/(Δt) = (Δ[HCl])/(Δt) = (Δ[HOCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/d1c898ea947b5f4b09c546231dd05230.png)
Construct the rate of reaction expression for: H_2O + Cl_2 ⟶ HCl + HOCl 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_2O + Cl_2 ⟶ HCl + HOCl 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_2O | 1 | -1 Cl_2 | 1 | -1 HCl | 1 | 1 HOCl | 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_2O | 1 | -1 | -(Δ[H2O])/(Δt) Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) HCl | 1 | 1 | (Δ[HCl])/(Δt) HOCl | 1 | 1 | (Δ[HOCl])/(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[H2O])/(Δt) = -(Δ[Cl2])/(Δt) = (Δ[HCl])/(Δt) = (Δ[HOCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| water | chlorine | hydrogen chloride | hypochlorous acid formula | H_2O | Cl_2 | HCl | HOCl Hill formula | H_2O | Cl_2 | ClH | ClHO name | water | chlorine | hydrogen chloride | hypochlorous acid IUPAC name | water | molecular chlorine | hydrogen chloride | hypochlorous acid](../image_source/4c48161d3ecfb6ff5a7c5b09b1eea9ed.png)
| water | chlorine | hydrogen chloride | hypochlorous acid formula | H_2O | Cl_2 | HCl | HOCl Hill formula | H_2O | Cl_2 | ClH | ClHO name | water | chlorine | hydrogen chloride | hypochlorous acid IUPAC name | water | molecular chlorine | hydrogen chloride | hypochlorous acid