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NaOH + Hg2Cl2 + SbCl3 = H2O + NaCl + Hg + NaSbO3

Input interpretation

NaOH sodium hydroxide + Hg_2Cl_2 mercury(I) chloride + SbCl_3 antimony(III) chloride ⟶ H_2O water + NaCl sodium chloride + Hg mercury + NaSbO3
NaOH sodium hydroxide + Hg_2Cl_2 mercury(I) chloride + SbCl_3 antimony(III) chloride ⟶ H_2O water + NaCl sodium chloride + Hg mercury + NaSbO3

Balanced equation

Balance the chemical equation algebraically: NaOH + Hg_2Cl_2 + SbCl_3 ⟶ H_2O + NaCl + Hg + NaSbO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Hg_2Cl_2 + c_3 SbCl_3 ⟶ c_4 H_2O + c_5 NaCl + c_6 Hg + c_7 NaSbO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Cl, Hg and Sb: H: | c_1 = 2 c_4 Na: | c_1 = c_5 + c_7 O: | c_1 = c_4 + 3 c_7 Cl: | 2 c_2 + 3 c_3 = c_5 Hg: | 2 c_2 = c_6 Sb: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 1 c_3 = 1 c_4 = 3 c_5 = 5 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 NaOH + Hg_2Cl_2 + SbCl_3 ⟶ 3 H_2O + 5 NaCl + 2 Hg + NaSbO3
Balance the chemical equation algebraically: NaOH + Hg_2Cl_2 + SbCl_3 ⟶ H_2O + NaCl + Hg + NaSbO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Hg_2Cl_2 + c_3 SbCl_3 ⟶ c_4 H_2O + c_5 NaCl + c_6 Hg + c_7 NaSbO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Cl, Hg and Sb: H: | c_1 = 2 c_4 Na: | c_1 = c_5 + c_7 O: | c_1 = c_4 + 3 c_7 Cl: | 2 c_2 + 3 c_3 = c_5 Hg: | 2 c_2 = c_6 Sb: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 1 c_3 = 1 c_4 = 3 c_5 = 5 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 NaOH + Hg_2Cl_2 + SbCl_3 ⟶ 3 H_2O + 5 NaCl + 2 Hg + NaSbO3

Structures

+ + ⟶ + + + NaSbO3
+ + ⟶ + + + NaSbO3

Names

sodium hydroxide + mercury(I) chloride + antimony(III) chloride ⟶ water + sodium chloride + mercury + NaSbO3
sodium hydroxide + mercury(I) chloride + antimony(III) chloride ⟶ water + sodium chloride + mercury + NaSbO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + Hg_2Cl_2 + SbCl_3 ⟶ H_2O + NaCl + Hg + NaSbO3 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 NaOH + Hg_2Cl_2 + SbCl_3 ⟶ 3 H_2O + 5 NaCl + 2 Hg + NaSbO3 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 NaOH | 6 | -6 Hg_2Cl_2 | 1 | -1 SbCl_3 | 1 | -1 H_2O | 3 | 3 NaCl | 5 | 5 Hg | 2 | 2 NaSbO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 6 | -6 | ([NaOH])^(-6) Hg_2Cl_2 | 1 | -1 | ([Hg2Cl2])^(-1) SbCl_3 | 1 | -1 | ([SbCl3])^(-1) H_2O | 3 | 3 | ([H2O])^3 NaCl | 5 | 5 | ([NaCl])^5 Hg | 2 | 2 | ([Hg])^2 NaSbO3 | 1 | 1 | [NaSbO3] 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 = ([NaOH])^(-6) ([Hg2Cl2])^(-1) ([SbCl3])^(-1) ([H2O])^3 ([NaCl])^5 ([Hg])^2 [NaSbO3] = (([H2O])^3 ([NaCl])^5 ([Hg])^2 [NaSbO3])/(([NaOH])^6 [Hg2Cl2] [SbCl3])
Construct the equilibrium constant, K, expression for: NaOH + Hg_2Cl_2 + SbCl_3 ⟶ H_2O + NaCl + Hg + NaSbO3 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 NaOH + Hg_2Cl_2 + SbCl_3 ⟶ 3 H_2O + 5 NaCl + 2 Hg + NaSbO3 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 NaOH | 6 | -6 Hg_2Cl_2 | 1 | -1 SbCl_3 | 1 | -1 H_2O | 3 | 3 NaCl | 5 | 5 Hg | 2 | 2 NaSbO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 6 | -6 | ([NaOH])^(-6) Hg_2Cl_2 | 1 | -1 | ([Hg2Cl2])^(-1) SbCl_3 | 1 | -1 | ([SbCl3])^(-1) H_2O | 3 | 3 | ([H2O])^3 NaCl | 5 | 5 | ([NaCl])^5 Hg | 2 | 2 | ([Hg])^2 NaSbO3 | 1 | 1 | [NaSbO3] 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 = ([NaOH])^(-6) ([Hg2Cl2])^(-1) ([SbCl3])^(-1) ([H2O])^3 ([NaCl])^5 ([Hg])^2 [NaSbO3] = (([H2O])^3 ([NaCl])^5 ([Hg])^2 [NaSbO3])/(([NaOH])^6 [Hg2Cl2] [SbCl3])

Rate of reaction

Construct the rate of reaction expression for: NaOH + Hg_2Cl_2 + SbCl_3 ⟶ H_2O + NaCl + Hg + NaSbO3 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 NaOH + Hg_2Cl_2 + SbCl_3 ⟶ 3 H_2O + 5 NaCl + 2 Hg + NaSbO3 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 NaOH | 6 | -6 Hg_2Cl_2 | 1 | -1 SbCl_3 | 1 | -1 H_2O | 3 | 3 NaCl | 5 | 5 Hg | 2 | 2 NaSbO3 | 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 NaOH | 6 | -6 | -1/6 (Δ[NaOH])/(Δt) Hg_2Cl_2 | 1 | -1 | -(Δ[Hg2Cl2])/(Δt) SbCl_3 | 1 | -1 | -(Δ[SbCl3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NaCl | 5 | 5 | 1/5 (Δ[NaCl])/(Δt) Hg | 2 | 2 | 1/2 (Δ[Hg])/(Δt) NaSbO3 | 1 | 1 | (Δ[NaSbO3])/(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[NaOH])/(Δt) = -(Δ[Hg2Cl2])/(Δt) = -(Δ[SbCl3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/5 (Δ[NaCl])/(Δt) = 1/2 (Δ[Hg])/(Δt) = (Δ[NaSbO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + Hg_2Cl_2 + SbCl_3 ⟶ H_2O + NaCl + Hg + NaSbO3 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 NaOH + Hg_2Cl_2 + SbCl_3 ⟶ 3 H_2O + 5 NaCl + 2 Hg + NaSbO3 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 NaOH | 6 | -6 Hg_2Cl_2 | 1 | -1 SbCl_3 | 1 | -1 H_2O | 3 | 3 NaCl | 5 | 5 Hg | 2 | 2 NaSbO3 | 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 NaOH | 6 | -6 | -1/6 (Δ[NaOH])/(Δt) Hg_2Cl_2 | 1 | -1 | -(Δ[Hg2Cl2])/(Δt) SbCl_3 | 1 | -1 | -(Δ[SbCl3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NaCl | 5 | 5 | 1/5 (Δ[NaCl])/(Δt) Hg | 2 | 2 | 1/2 (Δ[Hg])/(Δt) NaSbO3 | 1 | 1 | (Δ[NaSbO3])/(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[NaOH])/(Δt) = -(Δ[Hg2Cl2])/(Δt) = -(Δ[SbCl3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/5 (Δ[NaCl])/(Δt) = 1/2 (Δ[Hg])/(Δt) = (Δ[NaSbO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | mercury(I) chloride | antimony(III) chloride | water | sodium chloride | mercury | NaSbO3 formula | NaOH | Hg_2Cl_2 | SbCl_3 | H_2O | NaCl | Hg | NaSbO3 Hill formula | HNaO | Cl_2Hg_2 | Cl_3Sb | H_2O | ClNa | Hg | NaO3Sb name | sodium hydroxide | mercury(I) chloride | antimony(III) chloride | water | sodium chloride | mercury | IUPAC name | sodium hydroxide | chloromercury | trichlorostibane | water | sodium chloride | mercury |
| sodium hydroxide | mercury(I) chloride | antimony(III) chloride | water | sodium chloride | mercury | NaSbO3 formula | NaOH | Hg_2Cl_2 | SbCl_3 | H_2O | NaCl | Hg | NaSbO3 Hill formula | HNaO | Cl_2Hg_2 | Cl_3Sb | H_2O | ClNa | Hg | NaO3Sb name | sodium hydroxide | mercury(I) chloride | antimony(III) chloride | water | sodium chloride | mercury | IUPAC name | sodium hydroxide | chloromercury | trichlorostibane | water | sodium chloride | mercury |

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