Input interpretation
![HCl hydrogen chloride + NaOCl sodium hypochlorite ⟶ H_2O water + Cl_2 chlorine + NaCl sodium chloride](../image_source/aaa99617dd81e378388b0975e6e5fc35.png)
HCl hydrogen chloride + NaOCl sodium hypochlorite ⟶ H_2O water + Cl_2 chlorine + NaCl sodium chloride
Balanced equation
![Balance the chemical equation algebraically: HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaOCl ⟶ c_3 H_2O + c_4 Cl_2 + c_5 NaCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na and O: Cl: | c_1 + c_2 = 2 c_4 + c_5 H: | c_1 = 2 c_3 Na: | c_2 = c_5 O: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl](../image_source/4b3cf131f7bd62ce8003059dbd88dc4b.png)
Balance the chemical equation algebraically: HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaOCl ⟶ c_3 H_2O + c_4 Cl_2 + c_5 NaCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na and O: Cl: | c_1 + c_2 = 2 c_4 + c_5 H: | c_1 = 2 c_3 Na: | c_2 = c_5 O: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl
Structures
![+ ⟶ + +](../image_source/cb35f99c88cdffd0d15b5da744b5dfbe.png)
+ ⟶ + +
Names
![hydrogen chloride + sodium hypochlorite ⟶ water + chlorine + sodium chloride](../image_source/b3d663e98a5fc0514c26547d7447180f.png)
hydrogen chloride + sodium hypochlorite ⟶ water + chlorine + sodium chloride
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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: 2 HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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 | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 NaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) NaOCl | 1 | -1 | ([NaOCl])^(-1) H_2O | 1 | 1 | [H2O] Cl_2 | 1 | 1 | [Cl2] NaCl | 1 | 1 | [NaCl] 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])^(-2) ([NaOCl])^(-1) [H2O] [Cl2] [NaCl] = ([H2O] [Cl2] [NaCl])/(([HCl])^2 [NaOCl])](../image_source/d22f6f946a44d632d971c75ef4b36c45.png)
Construct the equilibrium constant, K, expression for: HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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: 2 HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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 | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 NaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) NaOCl | 1 | -1 | ([NaOCl])^(-1) H_2O | 1 | 1 | [H2O] Cl_2 | 1 | 1 | [Cl2] NaCl | 1 | 1 | [NaCl] 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])^(-2) ([NaOCl])^(-1) [H2O] [Cl2] [NaCl] = ([H2O] [Cl2] [NaCl])/(([HCl])^2 [NaOCl])
Rate of reaction
![Construct the rate of reaction expression for: HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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: 2 HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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 | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 NaCl | 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[NaOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = (Δ[NaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/bb108fdab5dd06ae4986b7ca6cdfa533.png)
Construct the rate of reaction expression for: HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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: 2 HCl + NaOCl ⟶ H_2O + Cl_2 + NaCl 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 | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 Cl_2 | 1 | 1 NaCl | 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cl_2 | 1 | 1 | (Δ[Cl2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[NaOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cl2])/(Δt) = (Δ[NaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen chloride | sodium hypochlorite | water | chlorine | sodium chloride formula | HCl | NaOCl | H_2O | Cl_2 | NaCl Hill formula | ClH | ClNaO | H_2O | Cl_2 | ClNa name | hydrogen chloride | sodium hypochlorite | water | chlorine | sodium chloride IUPAC name | hydrogen chloride | sodium hypochlorite | water | molecular chlorine | sodium chloride](../image_source/c7f4bc15f5d0ee71a0053d636b090f34.png)
| hydrogen chloride | sodium hypochlorite | water | chlorine | sodium chloride formula | HCl | NaOCl | H_2O | Cl_2 | NaCl Hill formula | ClH | ClNaO | H_2O | Cl_2 | ClNa name | hydrogen chloride | sodium hypochlorite | water | chlorine | sodium chloride IUPAC name | hydrogen chloride | sodium hypochlorite | water | molecular chlorine | sodium chloride
Substance properties
![| hydrogen chloride | sodium hypochlorite | water | chlorine | sodium chloride molar mass | 36.46 g/mol | 74.44 g/mol | 18.015 g/mol | 70.9 g/mol | 58.44 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | -6 °C | 0 °C | -101 °C | 801 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | 1413 °C density | 0.00149 g/cm^3 (at 25 °C) | 1.11 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 2.16 g/cm^3 solubility in water | miscible | miscible | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | | odorless](../image_source/33e77715a13443d80d7c57b13ca3fa34.png)
| hydrogen chloride | sodium hypochlorite | water | chlorine | sodium chloride molar mass | 36.46 g/mol | 74.44 g/mol | 18.015 g/mol | 70.9 g/mol | 58.44 g/mol phase | gas (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | -6 °C | 0 °C | -101 °C | 801 °C boiling point | -85 °C | | 99.9839 °C | -34 °C | 1413 °C density | 0.00149 g/cm^3 (at 25 °C) | 1.11 g/cm^3 | 1 g/cm^3 | 0.003214 g/cm^3 (at 0 °C) | 2.16 g/cm^3 solubility in water | miscible | miscible | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | | odorless
Units