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H2O + Cl2 + Ca3P2 = HCl + CaCl2 + H3PO4

Input interpretation

H_2O water + Cl_2 chlorine + Ca_3P_2 calcium phosphide ⟶ HCl hydrogen chloride + CaCl_2 calcium chloride + H_3PO_4 phosphoric acid
H_2O water + Cl_2 chlorine + Ca_3P_2 calcium phosphide ⟶ HCl hydrogen chloride + CaCl_2 calcium chloride + H_3PO_4 phosphoric acid

Balanced equation

Balance the chemical equation algebraically: H_2O + Cl_2 + Ca_3P_2 ⟶ HCl + CaCl_2 + H_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Ca_3P_2 ⟶ c_4 HCl + c_5 CaCl_2 + c_6 H_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Ca and P: H: | 2 c_1 = c_4 + 3 c_6 O: | c_1 = 4 c_6 Cl: | 2 c_2 = c_4 + 2 c_5 Ca: | 3 c_3 = c_5 P: | 2 c_3 = c_6 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 = 8 c_2 = 8 c_3 = 1 c_4 = 10 c_5 = 3 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2O + 8 Cl_2 + Ca_3P_2 ⟶ 10 HCl + 3 CaCl_2 + 2 H_3PO_4
Balance the chemical equation algebraically: H_2O + Cl_2 + Ca_3P_2 ⟶ HCl + CaCl_2 + H_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Ca_3P_2 ⟶ c_4 HCl + c_5 CaCl_2 + c_6 H_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Ca and P: H: | 2 c_1 = c_4 + 3 c_6 O: | c_1 = 4 c_6 Cl: | 2 c_2 = c_4 + 2 c_5 Ca: | 3 c_3 = c_5 P: | 2 c_3 = c_6 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 = 8 c_2 = 8 c_3 = 1 c_4 = 10 c_5 = 3 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2O + 8 Cl_2 + Ca_3P_2 ⟶ 10 HCl + 3 CaCl_2 + 2 H_3PO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + chlorine + calcium phosphide ⟶ hydrogen chloride + calcium chloride + phosphoric acid
water + chlorine + calcium phosphide ⟶ hydrogen chloride + calcium chloride + phosphoric acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Ca_3P_2 ⟶ HCl + CaCl_2 + H_3PO_4 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 H_2O + 8 Cl_2 + Ca_3P_2 ⟶ 10 HCl + 3 CaCl_2 + 2 H_3PO_4 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 | 8 | -8 Cl_2 | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 10 | 10 CaCl_2 | 3 | 3 H_3PO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 8 | -8 | ([H2O])^(-8) Cl_2 | 8 | -8 | ([Cl2])^(-8) Ca_3P_2 | 1 | -1 | ([Ca3P2])^(-1) HCl | 10 | 10 | ([HCl])^10 CaCl_2 | 3 | 3 | ([CaCl2])^3 H_3PO_4 | 2 | 2 | ([H3PO4])^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 = ([H2O])^(-8) ([Cl2])^(-8) ([Ca3P2])^(-1) ([HCl])^10 ([CaCl2])^3 ([H3PO4])^2 = (([HCl])^10 ([CaCl2])^3 ([H3PO4])^2)/(([H2O])^8 ([Cl2])^8 [Ca3P2])
Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Ca_3P_2 ⟶ HCl + CaCl_2 + H_3PO_4 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 H_2O + 8 Cl_2 + Ca_3P_2 ⟶ 10 HCl + 3 CaCl_2 + 2 H_3PO_4 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 | 8 | -8 Cl_2 | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 10 | 10 CaCl_2 | 3 | 3 H_3PO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 8 | -8 | ([H2O])^(-8) Cl_2 | 8 | -8 | ([Cl2])^(-8) Ca_3P_2 | 1 | -1 | ([Ca3P2])^(-1) HCl | 10 | 10 | ([HCl])^10 CaCl_2 | 3 | 3 | ([CaCl2])^3 H_3PO_4 | 2 | 2 | ([H3PO4])^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 = ([H2O])^(-8) ([Cl2])^(-8) ([Ca3P2])^(-1) ([HCl])^10 ([CaCl2])^3 ([H3PO4])^2 = (([HCl])^10 ([CaCl2])^3 ([H3PO4])^2)/(([H2O])^8 ([Cl2])^8 [Ca3P2])

Rate of reaction

Construct the rate of reaction expression for: H_2O + Cl_2 + Ca_3P_2 ⟶ HCl + CaCl_2 + H_3PO_4 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 H_2O + 8 Cl_2 + Ca_3P_2 ⟶ 10 HCl + 3 CaCl_2 + 2 H_3PO_4 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 | 8 | -8 Cl_2 | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 10 | 10 CaCl_2 | 3 | 3 H_3PO_4 | 2 | 2 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 | 8 | -8 | -1/8 (Δ[H2O])/(Δt) Cl_2 | 8 | -8 | -1/8 (Δ[Cl2])/(Δt) Ca_3P_2 | 1 | -1 | -(Δ[Ca3P2])/(Δt) HCl | 10 | 10 | 1/10 (Δ[HCl])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(Δt) H_3PO_4 | 2 | 2 | 1/2 (Δ[H3PO4])/(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[H2O])/(Δt) = -1/8 (Δ[Cl2])/(Δt) = -(Δ[Ca3P2])/(Δt) = 1/10 (Δ[HCl])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) = 1/2 (Δ[H3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Cl_2 + Ca_3P_2 ⟶ HCl + CaCl_2 + H_3PO_4 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 H_2O + 8 Cl_2 + Ca_3P_2 ⟶ 10 HCl + 3 CaCl_2 + 2 H_3PO_4 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 | 8 | -8 Cl_2 | 8 | -8 Ca_3P_2 | 1 | -1 HCl | 10 | 10 CaCl_2 | 3 | 3 H_3PO_4 | 2 | 2 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 | 8 | -8 | -1/8 (Δ[H2O])/(Δt) Cl_2 | 8 | -8 | -1/8 (Δ[Cl2])/(Δt) Ca_3P_2 | 1 | -1 | -(Δ[Ca3P2])/(Δt) HCl | 10 | 10 | 1/10 (Δ[HCl])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(Δt) H_3PO_4 | 2 | 2 | 1/2 (Δ[H3PO4])/(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[H2O])/(Δt) = -1/8 (Δ[Cl2])/(Δt) = -(Δ[Ca3P2])/(Δt) = 1/10 (Δ[HCl])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) = 1/2 (Δ[H3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | chlorine | calcium phosphide | hydrogen chloride | calcium chloride | phosphoric acid formula | H_2O | Cl_2 | Ca_3P_2 | HCl | CaCl_2 | H_3PO_4 Hill formula | H_2O | Cl_2 | Ca_3P_2 | ClH | CaCl_2 | H_3O_4P name | water | chlorine | calcium phosphide | hydrogen chloride | calcium chloride | phosphoric acid IUPAC name | water | molecular chlorine | calcium phosphanidylidenecalcium | hydrogen chloride | calcium dichloride | phosphoric acid
| water | chlorine | calcium phosphide | hydrogen chloride | calcium chloride | phosphoric acid formula | H_2O | Cl_2 | Ca_3P_2 | HCl | CaCl_2 | H_3PO_4 Hill formula | H_2O | Cl_2 | Ca_3P_2 | ClH | CaCl_2 | H_3O_4P name | water | chlorine | calcium phosphide | hydrogen chloride | calcium chloride | phosphoric acid IUPAC name | water | molecular chlorine | calcium phosphanidylidenecalcium | hydrogen chloride | calcium dichloride | phosphoric acid

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