Search

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

Input interpretation

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

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + HgS ⟶ H_2O + S + 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 S + 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 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 1 c_3 = 3/2 c_4 = 2 c_5 = 3/2 c_6 = 1 c_7 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 12 c_2 = 2 c_3 = 3 c_4 = 4 c_5 = 3 c_6 = 2 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HCl + 2 HNO_3 + 3 HgS ⟶ 4 H_2O + 3 S + 2 NO + 3 H2HgCl4
Balance the chemical equation algebraically: HCl + HNO_3 + HgS ⟶ H_2O + S + 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 S + 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 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 1 c_3 = 3/2 c_4 = 2 c_5 = 3/2 c_6 = 1 c_7 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 12 c_2 = 2 c_3 = 3 c_4 = 4 c_5 = 3 c_6 = 2 c_7 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 12 HCl + 2 HNO_3 + 3 HgS ⟶ 4 H_2O + 3 S + 2 NO + 3 H2HgCl4

Structures

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

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + HgS ⟶ H_2O + S + 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: 12 HCl + 2 HNO_3 + 3 HgS ⟶ 4 H_2O + 3 S + 2 NO + 3 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 | 12 | -12 HNO_3 | 2 | -2 HgS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 H2HgCl4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 12 | -12 | ([HCl])^(-12) HNO_3 | 2 | -2 | ([HNO3])^(-2) HgS | 3 | -3 | ([HgS])^(-3) H_2O | 4 | 4 | ([H2O])^4 S | 3 | 3 | ([S])^3 NO | 2 | 2 | ([NO])^2 H2HgCl4 | 3 | 3 | ([H2HgCl4])^3 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])^(-12) ([HNO3])^(-2) ([HgS])^(-3) ([H2O])^4 ([S])^3 ([NO])^2 ([H2HgCl4])^3 = (([H2O])^4 ([S])^3 ([NO])^2 ([H2HgCl4])^3)/(([HCl])^12 ([HNO3])^2 ([HgS])^3)
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + HgS ⟶ H_2O + S + 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: 12 HCl + 2 HNO_3 + 3 HgS ⟶ 4 H_2O + 3 S + 2 NO + 3 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 | 12 | -12 HNO_3 | 2 | -2 HgS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 H2HgCl4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 12 | -12 | ([HCl])^(-12) HNO_3 | 2 | -2 | ([HNO3])^(-2) HgS | 3 | -3 | ([HgS])^(-3) H_2O | 4 | 4 | ([H2O])^4 S | 3 | 3 | ([S])^3 NO | 2 | 2 | ([NO])^2 H2HgCl4 | 3 | 3 | ([H2HgCl4])^3 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])^(-12) ([HNO3])^(-2) ([HgS])^(-3) ([H2O])^4 ([S])^3 ([NO])^2 ([H2HgCl4])^3 = (([H2O])^4 ([S])^3 ([NO])^2 ([H2HgCl4])^3)/(([HCl])^12 ([HNO3])^2 ([HgS])^3)

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + HgS ⟶ H_2O + S + 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: 12 HCl + 2 HNO_3 + 3 HgS ⟶ 4 H_2O + 3 S + 2 NO + 3 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 | 12 | -12 HNO_3 | 2 | -2 HgS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 H2HgCl4 | 3 | 3 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 | 12 | -12 | -1/12 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) HgS | 3 | -3 | -1/3 (Δ[HgS])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) H2HgCl4 | 3 | 3 | 1/3 (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 = -1/12 (Δ[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/3 (Δ[HgS])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/3 (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 + S + 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: 12 HCl + 2 HNO_3 + 3 HgS ⟶ 4 H_2O + 3 S + 2 NO + 3 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 | 12 | -12 HNO_3 | 2 | -2 HgS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 H2HgCl4 | 3 | 3 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 | 12 | -12 | -1/12 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) HgS | 3 | -3 | -1/3 (Δ[HgS])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) S | 3 | 3 | 1/3 (Δ[S])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) H2HgCl4 | 3 | 3 | 1/3 (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 = -1/12 (Δ[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/3 (Δ[HgS])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/3 (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 | mixed sulfur | nitric oxide | H2HgCl4 formula | HCl | HNO_3 | HgS | H_2O | S | NO | H2HgCl4 Hill formula | ClH | HNO_3 | HgS | H_2O | S | NO | H2Cl4Hg name | hydrogen chloride | nitric acid | mercury(II) sulfide | water | mixed sulfur | nitric oxide | IUPAC name | hydrogen chloride | nitric acid | thioxomercury | water | sulfur | nitric oxide |
| hydrogen chloride | nitric acid | mercury(II) sulfide | water | mixed sulfur | nitric oxide | H2HgCl4 formula | HCl | HNO_3 | HgS | H_2O | S | NO | H2HgCl4 Hill formula | ClH | HNO_3 | HgS | H_2O | S | NO | H2Cl4Hg name | hydrogen chloride | nitric acid | mercury(II) sulfide | water | mixed sulfur | nitric oxide | IUPAC name | hydrogen chloride | nitric acid | thioxomercury | water | sulfur | nitric oxide |

Random Queries

PubChem SID number of hafnium(IV) carbide
ions of perchloric acid vs lithium chloride
formula string of scandium(II) cation vs scandium(III) cation
apply range filter image cetineite
formula of 1,1,1-trichloroethane vs methylene chloride
density of 2-thienyllithium vs lead(II) oxalate
electron count of strong electrolytes
color of amber vs gmelinite-Na
ion class of hydrogen cation vs sodium cation
structure diagram of dicarboxylic acid functional group