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HCl + HNO3 + HgS = H2O + SO2 + NO + H2HgCl4

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + HgS mercury(II) sulfide ⟶ H_2O water + SO_2 sulfur dioxide + NO nitric oxide + H2HgCl4
HCl hydrogen chloride + HNO_3 nitric acid + HgS mercury(II) sulfide ⟶ H_2O water + SO_2 sulfur dioxide + NO nitric oxide + H2HgCl4

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + HgS ⟶ H_2O + SO_2 + NO + H2HgCl4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 HgS ⟶ c_4 H_2O + c_5 SO_2 + c_6 NO + c_7 H2HgCl4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O, Hg and S: Cl: | c_1 = 4 c_7 H: | c_1 + c_2 = 2 c_4 + 2 c_7 N: | c_2 = c_6 O: | 3 c_2 = c_4 + 2 c_5 + c_6 Hg: | c_3 = c_7 S: | c_3 = c_5 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 = 4 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + 2 HNO_3 + HgS ⟶ 2 H_2O + SO_2 + 2 NO + H2HgCl4
Balance the chemical equation algebraically: HCl + HNO_3 + HgS ⟶ H_2O + SO_2 + NO + H2HgCl4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 HgS ⟶ c_4 H_2O + c_5 SO_2 + c_6 NO + c_7 H2HgCl4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O, Hg and S: Cl: | c_1 = 4 c_7 H: | c_1 + c_2 = 2 c_4 + 2 c_7 N: | c_2 = c_6 O: | 3 c_2 = c_4 + 2 c_5 + c_6 Hg: | c_3 = c_7 S: | c_3 = c_5 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 = 4 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + 2 HNO_3 + HgS ⟶ 2 H_2O + SO_2 + 2 NO + H2HgCl4

Structures

+ + ⟶ + + + H2HgCl4
+ + ⟶ + + + H2HgCl4

Names

hydrogen chloride + nitric acid + mercury(II) sulfide ⟶ water + sulfur dioxide + nitric oxide + H2HgCl4
hydrogen chloride + nitric acid + mercury(II) sulfide ⟶ water + sulfur dioxide + nitric oxide + H2HgCl4

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + HgS ⟶ H_2O + SO_2 + NO + H2HgCl4 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: 4 HCl + 2 HNO_3 + HgS ⟶ 2 H_2O + SO_2 + 2 NO + H2HgCl4 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 | 4 | -4 HNO_3 | 2 | -2 HgS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 NO | 2 | 2 H2HgCl4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) HNO_3 | 2 | -2 | ([HNO3])^(-2) HgS | 1 | -1 | ([HgS])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] NO | 2 | 2 | ([NO])^2 H2HgCl4 | 1 | 1 | [H2HgCl4] 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])^(-4) ([HNO3])^(-2) ([HgS])^(-1) ([H2O])^2 [SO2] ([NO])^2 [H2HgCl4] = (([H2O])^2 [SO2] ([NO])^2 [H2HgCl4])/(([HCl])^4 ([HNO3])^2 [HgS])
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + HgS ⟶ H_2O + SO_2 + NO + H2HgCl4 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: 4 HCl + 2 HNO_3 + HgS ⟶ 2 H_2O + SO_2 + 2 NO + H2HgCl4 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 | 4 | -4 HNO_3 | 2 | -2 HgS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 NO | 2 | 2 H2HgCl4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) HNO_3 | 2 | -2 | ([HNO3])^(-2) HgS | 1 | -1 | ([HgS])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] NO | 2 | 2 | ([NO])^2 H2HgCl4 | 1 | 1 | [H2HgCl4] 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])^(-4) ([HNO3])^(-2) ([HgS])^(-1) ([H2O])^2 [SO2] ([NO])^2 [H2HgCl4] = (([H2O])^2 [SO2] ([NO])^2 [H2HgCl4])/(([HCl])^4 ([HNO3])^2 [HgS])

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + HgS ⟶ H_2O + SO_2 + NO + H2HgCl4 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: 4 HCl + 2 HNO_3 + HgS ⟶ 2 H_2O + SO_2 + 2 NO + H2HgCl4 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 | 4 | -4 HNO_3 | 2 | -2 HgS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 NO | 2 | 2 H2HgCl4 | 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 | 4 | -4 | -1/4 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) HgS | 1 | -1 | -(Δ[HgS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) H2HgCl4 | 1 | 1 | (Δ[H2HgCl4])/(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 = -1/4 (Δ[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -(Δ[HgS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[H2HgCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + HgS ⟶ H_2O + SO_2 + NO + H2HgCl4 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: 4 HCl + 2 HNO_3 + HgS ⟶ 2 H_2O + SO_2 + 2 NO + H2HgCl4 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 | 4 | -4 HNO_3 | 2 | -2 HgS | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 NO | 2 | 2 H2HgCl4 | 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 | 4 | -4 | -1/4 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) HgS | 1 | -1 | -(Δ[HgS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) H2HgCl4 | 1 | 1 | (Δ[H2HgCl4])/(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 = -1/4 (Δ[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -(Δ[HgS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[H2HgCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | mercury(II) sulfide | water | sulfur dioxide | nitric oxide | H2HgCl4 formula | HCl | HNO_3 | HgS | H_2O | SO_2 | NO | H2HgCl4 Hill formula | ClH | HNO_3 | HgS | H_2O | O_2S | NO | H2Cl4Hg name | hydrogen chloride | nitric acid | mercury(II) sulfide | water | sulfur dioxide | nitric oxide | IUPAC name | hydrogen chloride | nitric acid | thioxomercury | water | sulfur dioxide | nitric oxide |
| hydrogen chloride | nitric acid | mercury(II) sulfide | water | sulfur dioxide | nitric oxide | H2HgCl4 formula | HCl | HNO_3 | HgS | H_2O | SO_2 | NO | H2HgCl4 Hill formula | ClH | HNO_3 | HgS | H_2O | O_2S | NO | H2Cl4Hg name | hydrogen chloride | nitric acid | mercury(II) sulfide | water | sulfur dioxide | nitric oxide | IUPAC name | hydrogen chloride | nitric acid | thioxomercury | water | sulfur dioxide | nitric oxide |

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