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HCl + HNO3 + NH4ClO4 = H2O + Cl2 + N2O + HClO4

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + NH_4ClO_4 ammonium perchlorate ⟶ H_2O water + Cl_2 chlorine + N_2O nitrous oxide + HClO_4 perchloric acid
HCl hydrogen chloride + HNO_3 nitric acid + NH_4ClO_4 ammonium perchlorate ⟶ H_2O water + Cl_2 chlorine + N_2O nitrous oxide + HClO_4 perchloric acid

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + NH_4ClO_4 ⟶ H_2O + Cl_2 + N_2O + HClO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 NH_4ClO_4 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 N_2O + c_7 HClO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | c_1 + c_3 = 2 c_5 + c_7 H: | c_1 + c_2 + 4 c_3 = 2 c_4 + c_7 N: | c_2 + c_3 = 2 c_6 O: | 3 c_2 + 4 c_3 = c_4 + c_6 + 4 c_7 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_3 = 1 c_4 = 25/14 + (4 c_1)/7 + (3 c_2)/14 c_5 = 2/7 + (4 c_1)/7 - (2 c_2)/7 c_6 = c_2/2 + 1/2 c_7 = 3/7 - c_1/7 + (4 c_2)/7 The resulting system of equations is still underdetermined, so additional coefficients must be set arbitrarily. Set c_1 = 8 and c_2 = 3 and solve for the remaining coefficients: c_1 = 8 c_2 = 3 c_3 = 1 c_4 = 7 c_5 = 4 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HCl + 3 HNO_3 + NH_4ClO_4 ⟶ 7 H_2O + 4 Cl_2 + 2 N_2O + HClO_4
Balance the chemical equation algebraically: HCl + HNO_3 + NH_4ClO_4 ⟶ H_2O + Cl_2 + N_2O + HClO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 NH_4ClO_4 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 N_2O + c_7 HClO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | c_1 + c_3 = 2 c_5 + c_7 H: | c_1 + c_2 + 4 c_3 = 2 c_4 + c_7 N: | c_2 + c_3 = 2 c_6 O: | 3 c_2 + 4 c_3 = c_4 + c_6 + 4 c_7 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_3 = 1 c_4 = 25/14 + (4 c_1)/7 + (3 c_2)/14 c_5 = 2/7 + (4 c_1)/7 - (2 c_2)/7 c_6 = c_2/2 + 1/2 c_7 = 3/7 - c_1/7 + (4 c_2)/7 The resulting system of equations is still underdetermined, so additional coefficients must be set arbitrarily. Set c_1 = 8 and c_2 = 3 and solve for the remaining coefficients: c_1 = 8 c_2 = 3 c_3 = 1 c_4 = 7 c_5 = 4 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HCl + 3 HNO_3 + NH_4ClO_4 ⟶ 7 H_2O + 4 Cl_2 + 2 N_2O + HClO_4

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

hydrogen chloride + nitric acid + ammonium perchlorate ⟶ water + chlorine + nitrous oxide + perchloric acid
hydrogen chloride + nitric acid + ammonium perchlorate ⟶ water + chlorine + nitrous oxide + perchloric acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + NH_4ClO_4 ⟶ H_2O + Cl_2 + N_2O + HClO_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 HCl + 3 HNO_3 + NH_4ClO_4 ⟶ 7 H_2O + 4 Cl_2 + 2 N_2O + HClO_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 HCl | 8 | -8 HNO_3 | 3 | -3 NH_4ClO_4 | 1 | -1 H_2O | 7 | 7 Cl_2 | 4 | 4 N_2O | 2 | 2 HClO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 8 | -8 | ([HCl])^(-8) HNO_3 | 3 | -3 | ([HNO3])^(-3) NH_4ClO_4 | 1 | -1 | ([NH4ClO4])^(-1) H_2O | 7 | 7 | ([H2O])^7 Cl_2 | 4 | 4 | ([Cl2])^4 N_2O | 2 | 2 | ([N2O])^2 HClO_4 | 1 | 1 | [HClO4] 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])^(-8) ([HNO3])^(-3) ([NH4ClO4])^(-1) ([H2O])^7 ([Cl2])^4 ([N2O])^2 [HClO4] = (([H2O])^7 ([Cl2])^4 ([N2O])^2 [HClO4])/(([HCl])^8 ([HNO3])^3 [NH4ClO4])
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + NH_4ClO_4 ⟶ H_2O + Cl_2 + N_2O + HClO_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 HCl + 3 HNO_3 + NH_4ClO_4 ⟶ 7 H_2O + 4 Cl_2 + 2 N_2O + HClO_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 HCl | 8 | -8 HNO_3 | 3 | -3 NH_4ClO_4 | 1 | -1 H_2O | 7 | 7 Cl_2 | 4 | 4 N_2O | 2 | 2 HClO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 8 | -8 | ([HCl])^(-8) HNO_3 | 3 | -3 | ([HNO3])^(-3) NH_4ClO_4 | 1 | -1 | ([NH4ClO4])^(-1) H_2O | 7 | 7 | ([H2O])^7 Cl_2 | 4 | 4 | ([Cl2])^4 N_2O | 2 | 2 | ([N2O])^2 HClO_4 | 1 | 1 | [HClO4] 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])^(-8) ([HNO3])^(-3) ([NH4ClO4])^(-1) ([H2O])^7 ([Cl2])^4 ([N2O])^2 [HClO4] = (([H2O])^7 ([Cl2])^4 ([N2O])^2 [HClO4])/(([HCl])^8 ([HNO3])^3 [NH4ClO4])

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + NH_4ClO_4 ⟶ H_2O + Cl_2 + N_2O + HClO_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 HCl + 3 HNO_3 + NH_4ClO_4 ⟶ 7 H_2O + 4 Cl_2 + 2 N_2O + HClO_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 HCl | 8 | -8 HNO_3 | 3 | -3 NH_4ClO_4 | 1 | -1 H_2O | 7 | 7 Cl_2 | 4 | 4 N_2O | 2 | 2 HClO_4 | 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 | 8 | -8 | -1/8 (Δ[HCl])/(Δt) HNO_3 | 3 | -3 | -1/3 (Δ[HNO3])/(Δt) NH_4ClO_4 | 1 | -1 | -(Δ[NH4ClO4])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) Cl_2 | 4 | 4 | 1/4 (Δ[Cl2])/(Δt) N_2O | 2 | 2 | 1/2 (Δ[N2O])/(Δt) HClO_4 | 1 | 1 | (Δ[HClO4])/(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[HCl])/(Δt) = -1/3 (Δ[HNO3])/(Δt) = -(Δ[NH4ClO4])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/4 (Δ[Cl2])/(Δt) = 1/2 (Δ[N2O])/(Δt) = (Δ[HClO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + NH_4ClO_4 ⟶ H_2O + Cl_2 + N_2O + HClO_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 HCl + 3 HNO_3 + NH_4ClO_4 ⟶ 7 H_2O + 4 Cl_2 + 2 N_2O + HClO_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 HCl | 8 | -8 HNO_3 | 3 | -3 NH_4ClO_4 | 1 | -1 H_2O | 7 | 7 Cl_2 | 4 | 4 N_2O | 2 | 2 HClO_4 | 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 | 8 | -8 | -1/8 (Δ[HCl])/(Δt) HNO_3 | 3 | -3 | -1/3 (Δ[HNO3])/(Δt) NH_4ClO_4 | 1 | -1 | -(Δ[NH4ClO4])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) Cl_2 | 4 | 4 | 1/4 (Δ[Cl2])/(Δt) N_2O | 2 | 2 | 1/2 (Δ[N2O])/(Δt) HClO_4 | 1 | 1 | (Δ[HClO4])/(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[HCl])/(Δt) = -1/3 (Δ[HNO3])/(Δt) = -(Δ[NH4ClO4])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/4 (Δ[Cl2])/(Δt) = 1/2 (Δ[N2O])/(Δt) = (Δ[HClO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | ammonium perchlorate | water | chlorine | nitrous oxide | perchloric acid formula | HCl | HNO_3 | NH_4ClO_4 | H_2O | Cl_2 | N_2O | HClO_4 Hill formula | ClH | HNO_3 | ClH_4NO_4 | H_2O | Cl_2 | N_2O | ClHO_4 name | hydrogen chloride | nitric acid | ammonium perchlorate | water | chlorine | nitrous oxide | perchloric acid IUPAC name | hydrogen chloride | nitric acid | | water | molecular chlorine | nitrous oxide | perchloric acid
| hydrogen chloride | nitric acid | ammonium perchlorate | water | chlorine | nitrous oxide | perchloric acid formula | HCl | HNO_3 | NH_4ClO_4 | H_2O | Cl_2 | N_2O | HClO_4 Hill formula | ClH | HNO_3 | ClH_4NO_4 | H_2O | Cl_2 | N_2O | ClHO_4 name | hydrogen chloride | nitric acid | ammonium perchlorate | water | chlorine | nitrous oxide | perchloric acid IUPAC name | hydrogen chloride | nitric acid | | water | molecular chlorine | nitrous oxide | perchloric acid

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