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HCl + HNO3 + MnS = H2O + S + NO + MnCl2

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + MnS manganese sulfide ⟶ H_2O water + S mixed sulfur + NO nitric oxide + MnCl_2 manganese(II) chloride
HCl hydrogen chloride + HNO_3 nitric acid + MnS manganese sulfide ⟶ H_2O water + S mixed sulfur + NO nitric oxide + MnCl_2 manganese(II) chloride

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + MnS ⟶ H_2O + S + NO + MnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 MnS ⟶ c_4 H_2O + c_5 S + c_6 NO + c_7 MnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O, Mn and S: Cl: | c_1 = 2 c_7 H: | c_1 + c_2 = 2 c_4 N: | c_2 = c_6 O: | 3 c_2 = c_4 + c_6 Mn: | 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 = 3 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 = 6 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: | | 6 HCl + 2 HNO_3 + 3 MnS ⟶ 4 H_2O + 3 S + 2 NO + 3 MnCl_2
Balance the chemical equation algebraically: HCl + HNO_3 + MnS ⟶ H_2O + S + NO + MnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 MnS ⟶ c_4 H_2O + c_5 S + c_6 NO + c_7 MnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O, Mn and S: Cl: | c_1 = 2 c_7 H: | c_1 + c_2 = 2 c_4 N: | c_2 = c_6 O: | 3 c_2 = c_4 + c_6 Mn: | 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 = 3 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 = 6 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: | | 6 HCl + 2 HNO_3 + 3 MnS ⟶ 4 H_2O + 3 S + 2 NO + 3 MnCl_2

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + MnS ⟶ H_2O + S + NO + MnCl_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: 6 HCl + 2 HNO_3 + 3 MnS ⟶ 4 H_2O + 3 S + 2 NO + 3 MnCl_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 HCl | 6 | -6 HNO_3 | 2 | -2 MnS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 MnCl_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) HNO_3 | 2 | -2 | ([HNO3])^(-2) MnS | 3 | -3 | ([MnS])^(-3) H_2O | 4 | 4 | ([H2O])^4 S | 3 | 3 | ([S])^3 NO | 2 | 2 | ([NO])^2 MnCl_2 | 3 | 3 | ([MnCl2])^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])^(-6) ([HNO3])^(-2) ([MnS])^(-3) ([H2O])^4 ([S])^3 ([NO])^2 ([MnCl2])^3 = (([H2O])^4 ([S])^3 ([NO])^2 ([MnCl2])^3)/(([HCl])^6 ([HNO3])^2 ([MnS])^3)
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + MnS ⟶ H_2O + S + NO + MnCl_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: 6 HCl + 2 HNO_3 + 3 MnS ⟶ 4 H_2O + 3 S + 2 NO + 3 MnCl_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 HCl | 6 | -6 HNO_3 | 2 | -2 MnS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 MnCl_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) HNO_3 | 2 | -2 | ([HNO3])^(-2) MnS | 3 | -3 | ([MnS])^(-3) H_2O | 4 | 4 | ([H2O])^4 S | 3 | 3 | ([S])^3 NO | 2 | 2 | ([NO])^2 MnCl_2 | 3 | 3 | ([MnCl2])^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])^(-6) ([HNO3])^(-2) ([MnS])^(-3) ([H2O])^4 ([S])^3 ([NO])^2 ([MnCl2])^3 = (([H2O])^4 ([S])^3 ([NO])^2 ([MnCl2])^3)/(([HCl])^6 ([HNO3])^2 ([MnS])^3)

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + MnS ⟶ H_2O + S + NO + MnCl_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: 6 HCl + 2 HNO_3 + 3 MnS ⟶ 4 H_2O + 3 S + 2 NO + 3 MnCl_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 HCl | 6 | -6 HNO_3 | 2 | -2 MnS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 MnCl_2 | 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) MnS | 3 | -3 | -1/3 (Δ[MnS])/(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) MnCl_2 | 3 | 3 | 1/3 (Δ[MnCl2])/(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[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/3 (Δ[MnS])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/3 (Δ[MnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + MnS ⟶ H_2O + S + NO + MnCl_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: 6 HCl + 2 HNO_3 + 3 MnS ⟶ 4 H_2O + 3 S + 2 NO + 3 MnCl_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 HCl | 6 | -6 HNO_3 | 2 | -2 MnS | 3 | -3 H_2O | 4 | 4 S | 3 | 3 NO | 2 | 2 MnCl_2 | 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) MnS | 3 | -3 | -1/3 (Δ[MnS])/(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) MnCl_2 | 3 | 3 | 1/3 (Δ[MnCl2])/(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[HCl])/(Δt) = -1/2 (Δ[HNO3])/(Δt) = -1/3 (Δ[MnS])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/3 (Δ[S])/(Δt) = 1/2 (Δ[NO])/(Δt) = 1/3 (Δ[MnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | manganese sulfide | water | mixed sulfur | nitric oxide | manganese(II) chloride formula | HCl | HNO_3 | MnS | H_2O | S | NO | MnCl_2 Hill formula | ClH | HNO_3 | MnS | H_2O | S | NO | Cl_2Mn name | hydrogen chloride | nitric acid | manganese sulfide | water | mixed sulfur | nitric oxide | manganese(II) chloride IUPAC name | hydrogen chloride | nitric acid | | water | sulfur | nitric oxide | dichloromanganese
| hydrogen chloride | nitric acid | manganese sulfide | water | mixed sulfur | nitric oxide | manganese(II) chloride formula | HCl | HNO_3 | MnS | H_2O | S | NO | MnCl_2 Hill formula | ClH | HNO_3 | MnS | H_2O | S | NO | Cl_2Mn name | hydrogen chloride | nitric acid | manganese sulfide | water | mixed sulfur | nitric oxide | manganese(II) chloride IUPAC name | hydrogen chloride | nitric acid | | water | sulfur | nitric oxide | dichloromanganese

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