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HNO3 + Hg2I2 = H2O + I2 + NO2 + Hg(NO3)2

Input interpretation

HNO_3 nitric acid + Hg_2I_2 mercury(I) iodide ⟶ H_2O water + I_2 iodine + NO_2 nitrogen dioxide + Hg(NO_3)_2 mercury(II) nitrate
HNO_3 nitric acid + Hg_2I_2 mercury(I) iodide ⟶ H_2O water + I_2 iodine + NO_2 nitrogen dioxide + Hg(NO_3)_2 mercury(II) nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Hg_2I_2 ⟶ H_2O + I_2 + NO_2 + Hg(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Hg_2I_2 ⟶ c_3 H_2O + c_4 I_2 + c_5 NO_2 + c_6 Hg(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Hg and I: H: | c_1 = 2 c_3 N: | c_1 = c_5 + 2 c_6 O: | 3 c_1 = c_3 + 2 c_5 + 6 c_6 Hg: | 2 c_2 = c_6 I: | 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 = 4 c_4 = 1 c_5 = 4 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + Hg_2I_2 ⟶ 4 H_2O + I_2 + 4 NO_2 + 2 Hg(NO_3)_2
Balance the chemical equation algebraically: HNO_3 + Hg_2I_2 ⟶ H_2O + I_2 + NO_2 + Hg(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Hg_2I_2 ⟶ c_3 H_2O + c_4 I_2 + c_5 NO_2 + c_6 Hg(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Hg and I: H: | c_1 = 2 c_3 N: | c_1 = c_5 + 2 c_6 O: | 3 c_1 = c_3 + 2 c_5 + 6 c_6 Hg: | 2 c_2 = c_6 I: | 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 = 4 c_4 = 1 c_5 = 4 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HNO_3 + Hg_2I_2 ⟶ 4 H_2O + I_2 + 4 NO_2 + 2 Hg(NO_3)_2

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

nitric acid + mercury(I) iodide ⟶ water + iodine + nitrogen dioxide + mercury(II) nitrate
nitric acid + mercury(I) iodide ⟶ water + iodine + nitrogen dioxide + mercury(II) nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Hg_2I_2 ⟶ H_2O + I_2 + NO_2 + Hg(NO_3)_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 HNO_3 + Hg_2I_2 ⟶ 4 H_2O + I_2 + 4 NO_2 + 2 Hg(NO_3)_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 HNO_3 | 8 | -8 Hg_2I_2 | 1 | -1 H_2O | 4 | 4 I_2 | 1 | 1 NO_2 | 4 | 4 Hg(NO_3)_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) Hg_2I_2 | 1 | -1 | ([Hg2I2])^(-1) H_2O | 4 | 4 | ([H2O])^4 I_2 | 1 | 1 | [I2] NO_2 | 4 | 4 | ([NO2])^4 Hg(NO_3)_2 | 2 | 2 | ([Hg(NO3)2])^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 = ([HNO3])^(-8) ([Hg2I2])^(-1) ([H2O])^4 [I2] ([NO2])^4 ([Hg(NO3)2])^2 = (([H2O])^4 [I2] ([NO2])^4 ([Hg(NO3)2])^2)/(([HNO3])^8 [Hg2I2])
Construct the equilibrium constant, K, expression for: HNO_3 + Hg_2I_2 ⟶ H_2O + I_2 + NO_2 + Hg(NO_3)_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 HNO_3 + Hg_2I_2 ⟶ 4 H_2O + I_2 + 4 NO_2 + 2 Hg(NO_3)_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 HNO_3 | 8 | -8 Hg_2I_2 | 1 | -1 H_2O | 4 | 4 I_2 | 1 | 1 NO_2 | 4 | 4 Hg(NO_3)_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 8 | -8 | ([HNO3])^(-8) Hg_2I_2 | 1 | -1 | ([Hg2I2])^(-1) H_2O | 4 | 4 | ([H2O])^4 I_2 | 1 | 1 | [I2] NO_2 | 4 | 4 | ([NO2])^4 Hg(NO_3)_2 | 2 | 2 | ([Hg(NO3)2])^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 = ([HNO3])^(-8) ([Hg2I2])^(-1) ([H2O])^4 [I2] ([NO2])^4 ([Hg(NO3)2])^2 = (([H2O])^4 [I2] ([NO2])^4 ([Hg(NO3)2])^2)/(([HNO3])^8 [Hg2I2])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Hg_2I_2 ⟶ H_2O + I_2 + NO_2 + Hg(NO_3)_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 HNO_3 + Hg_2I_2 ⟶ 4 H_2O + I_2 + 4 NO_2 + 2 Hg(NO_3)_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 HNO_3 | 8 | -8 Hg_2I_2 | 1 | -1 H_2O | 4 | 4 I_2 | 1 | 1 NO_2 | 4 | 4 Hg(NO_3)_2 | 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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) Hg_2I_2 | 1 | -1 | -(Δ[Hg2I2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) NO_2 | 4 | 4 | 1/4 (Δ[NO2])/(Δt) Hg(NO_3)_2 | 2 | 2 | 1/2 (Δ[Hg(NO3)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[HNO3])/(Δt) = -(Δ[Hg2I2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[I2])/(Δt) = 1/4 (Δ[NO2])/(Δt) = 1/2 (Δ[Hg(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Hg_2I_2 ⟶ H_2O + I_2 + NO_2 + Hg(NO_3)_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 HNO_3 + Hg_2I_2 ⟶ 4 H_2O + I_2 + 4 NO_2 + 2 Hg(NO_3)_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 HNO_3 | 8 | -8 Hg_2I_2 | 1 | -1 H_2O | 4 | 4 I_2 | 1 | 1 NO_2 | 4 | 4 Hg(NO_3)_2 | 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 HNO_3 | 8 | -8 | -1/8 (Δ[HNO3])/(Δt) Hg_2I_2 | 1 | -1 | -(Δ[Hg2I2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) NO_2 | 4 | 4 | 1/4 (Δ[NO2])/(Δt) Hg(NO_3)_2 | 2 | 2 | 1/2 (Δ[Hg(NO3)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[HNO3])/(Δt) = -(Δ[Hg2I2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[I2])/(Δt) = 1/4 (Δ[NO2])/(Δt) = 1/2 (Δ[Hg(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | mercury(I) iodide | water | iodine | nitrogen dioxide | mercury(II) nitrate formula | HNO_3 | Hg_2I_2 | H_2O | I_2 | NO_2 | Hg(NO_3)_2 Hill formula | HNO_3 | Hg_2I_2 | H_2O | I_2 | NO_2 | HgN_2O_6 name | nitric acid | mercury(I) iodide | water | iodine | nitrogen dioxide | mercury(II) nitrate IUPAC name | nitric acid | iodomercury | water | molecular iodine | Nitrogen dioxide | mercury(+2) cation dinitrate
| nitric acid | mercury(I) iodide | water | iodine | nitrogen dioxide | mercury(II) nitrate formula | HNO_3 | Hg_2I_2 | H_2O | I_2 | NO_2 | Hg(NO_3)_2 Hill formula | HNO_3 | Hg_2I_2 | H_2O | I_2 | NO_2 | HgN_2O_6 name | nitric acid | mercury(I) iodide | water | iodine | nitrogen dioxide | mercury(II) nitrate IUPAC name | nitric acid | iodomercury | water | molecular iodine | Nitrogen dioxide | mercury(+2) cation dinitrate

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