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HClO + Ca3P2 = HCl + Ca3(PO4)2

Input interpretation

HOCl hypochlorous acid + Ca_3P_2 calcium phosphide ⟶ HCl hydrogen chloride + Ca_3(PO_4)_2 tricalcium diphosphate
HOCl hypochlorous acid + Ca_3P_2 calcium phosphide ⟶ HCl hydrogen chloride + Ca_3(PO_4)_2 tricalcium diphosphate

Balanced equation

Balance the chemical equation algebraically: HOCl + Ca_3P_2 ⟶ HCl + Ca_3(PO_4)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HOCl + c_2 Ca_3P_2 ⟶ c_3 HCl + c_4 Ca_3(PO_4)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O, Ca and P: Cl: | c_1 = c_3 H: | c_1 = c_3 O: | c_1 = 8 c_4 Ca: | 3 c_2 = 3 c_4 P: | 2 c_2 = 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 8 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HOCl + Ca_3P_2 ⟶ 8 HCl + Ca_3(PO_4)_2
Balance the chemical equation algebraically: HOCl + Ca_3P_2 ⟶ HCl + Ca_3(PO_4)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HOCl + c_2 Ca_3P_2 ⟶ c_3 HCl + c_4 Ca_3(PO_4)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O, Ca and P: Cl: | c_1 = c_3 H: | c_1 = c_3 O: | c_1 = 8 c_4 Ca: | 3 c_2 = 3 c_4 P: | 2 c_2 = 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 8 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HOCl + Ca_3P_2 ⟶ 8 HCl + Ca_3(PO_4)_2

Structures

+ ⟶ +
+ ⟶ +

Names

hypochlorous acid + calcium phosphide ⟶ hydrogen chloride + tricalcium diphosphate
hypochlorous acid + calcium phosphide ⟶ hydrogen chloride + tricalcium diphosphate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HOCl + Ca_3P_2 ⟶ HCl + Ca_3(PO_4)_2 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: 8 HOCl + Ca_3P_2 ⟶ 8 HCl + Ca_3(PO_4)_2 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 HOCl | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 8 | 8 Ca_3(PO_4)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HOCl | 8 | -8 | ([HOCl])^(-8) Ca_3P_2 | 1 | -1 | ([Ca3P2])^(-1) HCl | 8 | 8 | ([HCl])^8 Ca_3(PO_4)_2 | 1 | 1 | [Ca3(PO4)2] 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 = ([HOCl])^(-8) ([Ca3P2])^(-1) ([HCl])^8 [Ca3(PO4)2] = (([HCl])^8 [Ca3(PO4)2])/(([HOCl])^8 [Ca3P2])
Construct the equilibrium constant, K, expression for: HOCl + Ca_3P_2 ⟶ HCl + Ca_3(PO_4)_2 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: 8 HOCl + Ca_3P_2 ⟶ 8 HCl + Ca_3(PO_4)_2 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 HOCl | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 8 | 8 Ca_3(PO_4)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HOCl | 8 | -8 | ([HOCl])^(-8) Ca_3P_2 | 1 | -1 | ([Ca3P2])^(-1) HCl | 8 | 8 | ([HCl])^8 Ca_3(PO_4)_2 | 1 | 1 | [Ca3(PO4)2] 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 = ([HOCl])^(-8) ([Ca3P2])^(-1) ([HCl])^8 [Ca3(PO4)2] = (([HCl])^8 [Ca3(PO4)2])/(([HOCl])^8 [Ca3P2])

Rate of reaction

Construct the rate of reaction expression for: HOCl + Ca_3P_2 ⟶ HCl + Ca_3(PO_4)_2 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: 8 HOCl + Ca_3P_2 ⟶ 8 HCl + Ca_3(PO_4)_2 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 HOCl | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 8 | 8 Ca_3(PO_4)_2 | 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 HOCl | 8 | -8 | -1/8 (Δ[HOCl])/(Δt) Ca_3P_2 | 1 | -1 | -(Δ[Ca3P2])/(Δt) HCl | 8 | 8 | 1/8 (Δ[HCl])/(Δt) Ca_3(PO_4)_2 | 1 | 1 | (Δ[Ca3(PO4)2])/(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 = -1/8 (Δ[HOCl])/(Δt) = -(Δ[Ca3P2])/(Δt) = 1/8 (Δ[HCl])/(Δt) = (Δ[Ca3(PO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HOCl + Ca_3P_2 ⟶ HCl + Ca_3(PO_4)_2 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: 8 HOCl + Ca_3P_2 ⟶ 8 HCl + Ca_3(PO_4)_2 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 HOCl | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 8 | 8 Ca_3(PO_4)_2 | 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 HOCl | 8 | -8 | -1/8 (Δ[HOCl])/(Δt) Ca_3P_2 | 1 | -1 | -(Δ[Ca3P2])/(Δt) HCl | 8 | 8 | 1/8 (Δ[HCl])/(Δt) Ca_3(PO_4)_2 | 1 | 1 | (Δ[Ca3(PO4)2])/(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 = -1/8 (Δ[HOCl])/(Δt) = -(Δ[Ca3P2])/(Δt) = 1/8 (Δ[HCl])/(Δt) = (Δ[Ca3(PO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hypochlorous acid | calcium phosphide | hydrogen chloride | tricalcium diphosphate formula | HOCl | Ca_3P_2 | HCl | Ca_3(PO_4)_2 Hill formula | ClHO | Ca_3P_2 | ClH | Ca_3O_8P_2 name | hypochlorous acid | calcium phosphide | hydrogen chloride | tricalcium diphosphate IUPAC name | hypochlorous acid | calcium phosphanidylidenecalcium | hydrogen chloride | tricalcium diphosphate
| hypochlorous acid | calcium phosphide | hydrogen chloride | tricalcium diphosphate formula | HOCl | Ca_3P_2 | HCl | Ca_3(PO_4)_2 Hill formula | ClHO | Ca_3P_2 | ClH | Ca_3O_8P_2 name | hypochlorous acid | calcium phosphide | hydrogen chloride | tricalcium diphosphate IUPAC name | hypochlorous acid | calcium phosphanidylidenecalcium | hydrogen chloride | tricalcium diphosphate

Substance properties

| hypochlorous acid | calcium phosphide | hydrogen chloride | tricalcium diphosphate molar mass | 52.46 g/mol | 182.18 g/mol | 36.46 g/mol | 310.17 g/mol phase | | liquid (at STP) | gas (at STP) | melting point | | 0.16 °C | -114.17 °C | boiling point | | | -85 °C | density | | 2.51 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 3.14 g/cm^3 solubility in water | soluble | decomposes | miscible |
| hypochlorous acid | calcium phosphide | hydrogen chloride | tricalcium diphosphate molar mass | 52.46 g/mol | 182.18 g/mol | 36.46 g/mol | 310.17 g/mol phase | | liquid (at STP) | gas (at STP) | melting point | | 0.16 °C | -114.17 °C | boiling point | | | -85 °C | density | | 2.51 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 3.14 g/cm^3 solubility in water | soluble | decomposes | miscible |

Units

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