Search

Cl2 + Ca(OH)2 = HCl + CaCl2 + Ca(ClO3)2

Input interpretation

Cl_2 chlorine + Ca(OH)_2 calcium hydroxide ⟶ HCl hydrogen chloride + CaCl_2 calcium chloride + CaCl_2O_6 calcium chlorate
Cl_2 chlorine + Ca(OH)_2 calcium hydroxide ⟶ HCl hydrogen chloride + CaCl_2 calcium chloride + CaCl_2O_6 calcium chlorate

Balanced equation

Balance the chemical equation algebraically: Cl_2 + Ca(OH)_2 ⟶ HCl + CaCl_2 + CaCl_2O_6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Ca(OH)_2 ⟶ c_3 HCl + c_4 CaCl_2 + c_5 CaCl_2O_6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Ca, H and O: Cl: | 2 c_1 = c_3 + 2 c_4 + 2 c_5 Ca: | c_2 = c_4 + c_5 H: | 2 c_2 = c_3 O: | 2 c_2 = 6 c_5 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 3 c_3 = 6 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Cl_2 + 3 Ca(OH)_2 ⟶ 6 HCl + 2 CaCl_2 + CaCl_2O_6
Balance the chemical equation algebraically: Cl_2 + Ca(OH)_2 ⟶ HCl + CaCl_2 + CaCl_2O_6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Ca(OH)_2 ⟶ c_3 HCl + c_4 CaCl_2 + c_5 CaCl_2O_6 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Ca, H and O: Cl: | 2 c_1 = c_3 + 2 c_4 + 2 c_5 Ca: | c_2 = c_4 + c_5 H: | 2 c_2 = c_3 O: | 2 c_2 = 6 c_5 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 3 c_3 = 6 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Cl_2 + 3 Ca(OH)_2 ⟶ 6 HCl + 2 CaCl_2 + CaCl_2O_6

Structures

+ ⟶ + +
+ ⟶ + +

Names

chlorine + calcium hydroxide ⟶ hydrogen chloride + calcium chloride + calcium chlorate
chlorine + calcium hydroxide ⟶ hydrogen chloride + calcium chloride + calcium chlorate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + Ca(OH)_2 ⟶ HCl + CaCl_2 + CaCl_2O_6 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 Cl_2 + 3 Ca(OH)_2 ⟶ 6 HCl + 2 CaCl_2 + CaCl_2O_6 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 Cl_2 | 6 | -6 Ca(OH)_2 | 3 | -3 HCl | 6 | 6 CaCl_2 | 2 | 2 CaCl_2O_6 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 6 | -6 | ([Cl2])^(-6) Ca(OH)_2 | 3 | -3 | ([Ca(OH)2])^(-3) HCl | 6 | 6 | ([HCl])^6 CaCl_2 | 2 | 2 | ([CaCl2])^2 CaCl_2O_6 | 1 | 1 | [CaCl2O6] 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 = ([Cl2])^(-6) ([Ca(OH)2])^(-3) ([HCl])^6 ([CaCl2])^2 [CaCl2O6] = (([HCl])^6 ([CaCl2])^2 [CaCl2O6])/(([Cl2])^6 ([Ca(OH)2])^3)
Construct the equilibrium constant, K, expression for: Cl_2 + Ca(OH)_2 ⟶ HCl + CaCl_2 + CaCl_2O_6 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 Cl_2 + 3 Ca(OH)_2 ⟶ 6 HCl + 2 CaCl_2 + CaCl_2O_6 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 Cl_2 | 6 | -6 Ca(OH)_2 | 3 | -3 HCl | 6 | 6 CaCl_2 | 2 | 2 CaCl_2O_6 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 6 | -6 | ([Cl2])^(-6) Ca(OH)_2 | 3 | -3 | ([Ca(OH)2])^(-3) HCl | 6 | 6 | ([HCl])^6 CaCl_2 | 2 | 2 | ([CaCl2])^2 CaCl_2O_6 | 1 | 1 | [CaCl2O6] 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 = ([Cl2])^(-6) ([Ca(OH)2])^(-3) ([HCl])^6 ([CaCl2])^2 [CaCl2O6] = (([HCl])^6 ([CaCl2])^2 [CaCl2O6])/(([Cl2])^6 ([Ca(OH)2])^3)

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + Ca(OH)_2 ⟶ HCl + CaCl_2 + CaCl_2O_6 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 Cl_2 + 3 Ca(OH)_2 ⟶ 6 HCl + 2 CaCl_2 + CaCl_2O_6 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 Cl_2 | 6 | -6 Ca(OH)_2 | 3 | -3 HCl | 6 | 6 CaCl_2 | 2 | 2 CaCl_2O_6 | 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 Cl_2 | 6 | -6 | -1/6 (Δ[Cl2])/(Δt) Ca(OH)_2 | 3 | -3 | -1/3 (Δ[Ca(OH)2])/(Δt) HCl | 6 | 6 | 1/6 (Δ[HCl])/(Δt) CaCl_2 | 2 | 2 | 1/2 (Δ[CaCl2])/(Δt) CaCl_2O_6 | 1 | 1 | (Δ[CaCl2O6])/(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[Cl2])/(Δt) = -1/3 (Δ[Ca(OH)2])/(Δt) = 1/6 (Δ[HCl])/(Δt) = 1/2 (Δ[CaCl2])/(Δt) = (Δ[CaCl2O6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + Ca(OH)_2 ⟶ HCl + CaCl_2 + CaCl_2O_6 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 Cl_2 + 3 Ca(OH)_2 ⟶ 6 HCl + 2 CaCl_2 + CaCl_2O_6 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 Cl_2 | 6 | -6 Ca(OH)_2 | 3 | -3 HCl | 6 | 6 CaCl_2 | 2 | 2 CaCl_2O_6 | 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 Cl_2 | 6 | -6 | -1/6 (Δ[Cl2])/(Δt) Ca(OH)_2 | 3 | -3 | -1/3 (Δ[Ca(OH)2])/(Δt) HCl | 6 | 6 | 1/6 (Δ[HCl])/(Δt) CaCl_2 | 2 | 2 | 1/2 (Δ[CaCl2])/(Δt) CaCl_2O_6 | 1 | 1 | (Δ[CaCl2O6])/(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[Cl2])/(Δt) = -1/3 (Δ[Ca(OH)2])/(Δt) = 1/6 (Δ[HCl])/(Δt) = 1/2 (Δ[CaCl2])/(Δt) = (Δ[CaCl2O6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | calcium hydroxide | hydrogen chloride | calcium chloride | calcium chlorate formula | Cl_2 | Ca(OH)_2 | HCl | CaCl_2 | CaCl_2O_6 Hill formula | Cl_2 | CaH_2O_2 | ClH | CaCl_2 | CaCl_2O_6 name | chlorine | calcium hydroxide | hydrogen chloride | calcium chloride | calcium chlorate IUPAC name | molecular chlorine | calcium dihydroxide | hydrogen chloride | calcium dichloride | calcium dichlorate
| chlorine | calcium hydroxide | hydrogen chloride | calcium chloride | calcium chlorate formula | Cl_2 | Ca(OH)_2 | HCl | CaCl_2 | CaCl_2O_6 Hill formula | Cl_2 | CaH_2O_2 | ClH | CaCl_2 | CaCl_2O_6 name | chlorine | calcium hydroxide | hydrogen chloride | calcium chloride | calcium chlorate IUPAC name | molecular chlorine | calcium dihydroxide | hydrogen chloride | calcium dichloride | calcium dichlorate

Substance properties

| chlorine | calcium hydroxide | hydrogen chloride | calcium chloride | calcium chlorate molar mass | 70.9 g/mol | 74.092 g/mol | 36.46 g/mol | 111 g/mol | 207 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) melting point | -101 °C | 550 °C | -114.17 °C | 772 °C | 325 °C boiling point | -34 °C | | -85 °C | | density | 0.003214 g/cm^3 (at 0 °C) | 2.24 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 2.15 g/cm^3 | 2.71 g/cm^3 solubility in water | | slightly soluble | miscible | soluble | soluble odor | | odorless | | |
| chlorine | calcium hydroxide | hydrogen chloride | calcium chloride | calcium chlorate molar mass | 70.9 g/mol | 74.092 g/mol | 36.46 g/mol | 111 g/mol | 207 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) melting point | -101 °C | 550 °C | -114.17 °C | 772 °C | 325 °C boiling point | -34 °C | | -85 °C | | density | 0.003214 g/cm^3 (at 0 °C) | 2.24 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 2.15 g/cm^3 | 2.71 g/cm^3 solubility in water | | slightly soluble | miscible | soluble | soluble odor | | odorless | | |

Units

Random Queries

structure diagram of tin(II) cation vs carbonate anion
atomic radius of hafnium vs manganese
formula string of permanganate anion
chemical types sodium tetraborate tetrahydrate
CAS number of acetic acid vs chloroacetic acid
isotope abundances of boron
group of tungsten
molar mass of rubidium chloride
alternate names of mercury(II) cation
dielectric constant of propylene glycol