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HCl + H2O2 + CuS = H2O + S + CuCl2

Input interpretation

HCl hydrogen chloride + H_2O_2 hydrogen peroxide + CuS cupric sulfide ⟶ H_2O water + S mixed sulfur + CuCl_2 copper(II) chloride
HCl hydrogen chloride + H_2O_2 hydrogen peroxide + CuS cupric sulfide ⟶ H_2O water + S mixed sulfur + CuCl_2 copper(II) chloride

Balanced equation

Balance the chemical equation algebraically: HCl + H_2O_2 + CuS ⟶ H_2O + S + CuCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 H_2O_2 + c_3 CuS ⟶ c_4 H_2O + c_5 S + c_6 CuCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O, Cu and S: Cl: | c_1 = 2 c_6 H: | c_1 + 2 c_2 = 2 c_4 O: | 2 c_2 = c_4 Cu: | c_3 = c_6 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 = 2 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + H_2O_2 + CuS ⟶ 2 H_2O + S + CuCl_2
Balance the chemical equation algebraically: HCl + H_2O_2 + CuS ⟶ H_2O + S + CuCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 H_2O_2 + c_3 CuS ⟶ c_4 H_2O + c_5 S + c_6 CuCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O, Cu and S: Cl: | c_1 = 2 c_6 H: | c_1 + 2 c_2 = 2 c_4 O: | 2 c_2 = c_4 Cu: | c_3 = c_6 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 = 2 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + H_2O_2 + CuS ⟶ 2 H_2O + S + CuCl_2

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

hydrogen chloride + hydrogen peroxide + cupric sulfide ⟶ water + mixed sulfur + copper(II) chloride
hydrogen chloride + hydrogen peroxide + cupric sulfide ⟶ water + mixed sulfur + copper(II) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + H_2O_2 + CuS ⟶ H_2O + S + CuCl_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: 2 HCl + H_2O_2 + CuS ⟶ 2 H_2O + S + CuCl_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 | 2 | -2 H_2O_2 | 1 | -1 CuS | 1 | -1 H_2O | 2 | 2 S | 1 | 1 CuCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) CuS | 1 | -1 | ([CuS])^(-1) H_2O | 2 | 2 | ([H2O])^2 S | 1 | 1 | [S] CuCl_2 | 1 | 1 | [CuCl2] 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])^(-2) ([H2O2])^(-1) ([CuS])^(-1) ([H2O])^2 [S] [CuCl2] = (([H2O])^2 [S] [CuCl2])/(([HCl])^2 [H2O2] [CuS])
Construct the equilibrium constant, K, expression for: HCl + H_2O_2 + CuS ⟶ H_2O + S + CuCl_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: 2 HCl + H_2O_2 + CuS ⟶ 2 H_2O + S + CuCl_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 | 2 | -2 H_2O_2 | 1 | -1 CuS | 1 | -1 H_2O | 2 | 2 S | 1 | 1 CuCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) CuS | 1 | -1 | ([CuS])^(-1) H_2O | 2 | 2 | ([H2O])^2 S | 1 | 1 | [S] CuCl_2 | 1 | 1 | [CuCl2] 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])^(-2) ([H2O2])^(-1) ([CuS])^(-1) ([H2O])^2 [S] [CuCl2] = (([H2O])^2 [S] [CuCl2])/(([HCl])^2 [H2O2] [CuS])

Rate of reaction

Construct the rate of reaction expression for: HCl + H_2O_2 + CuS ⟶ H_2O + S + CuCl_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: 2 HCl + H_2O_2 + CuS ⟶ 2 H_2O + S + CuCl_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 | 2 | -2 H_2O_2 | 1 | -1 CuS | 1 | -1 H_2O | 2 | 2 S | 1 | 1 CuCl_2 | 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) CuS | 1 | -1 | -(Δ[CuS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) CuCl_2 | 1 | 1 | (Δ[CuCl2])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[H2O2])/(Δt) = -(Δ[CuS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[S])/(Δt) = (Δ[CuCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + H_2O_2 + CuS ⟶ H_2O + S + CuCl_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: 2 HCl + H_2O_2 + CuS ⟶ 2 H_2O + S + CuCl_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 | 2 | -2 H_2O_2 | 1 | -1 CuS | 1 | -1 H_2O | 2 | 2 S | 1 | 1 CuCl_2 | 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) CuS | 1 | -1 | -(Δ[CuS])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) CuCl_2 | 1 | 1 | (Δ[CuCl2])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[H2O2])/(Δt) = -(Δ[CuS])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[S])/(Δt) = (Δ[CuCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | hydrogen peroxide | cupric sulfide | water | mixed sulfur | copper(II) chloride formula | HCl | H_2O_2 | CuS | H_2O | S | CuCl_2 Hill formula | ClH | H_2O_2 | CuS | H_2O | S | Cl_2Cu name | hydrogen chloride | hydrogen peroxide | cupric sulfide | water | mixed sulfur | copper(II) chloride IUPAC name | hydrogen chloride | hydrogen peroxide | | water | sulfur | dichlorocopper
| hydrogen chloride | hydrogen peroxide | cupric sulfide | water | mixed sulfur | copper(II) chloride formula | HCl | H_2O_2 | CuS | H_2O | S | CuCl_2 Hill formula | ClH | H_2O_2 | CuS | H_2O | S | Cl_2Cu name | hydrogen chloride | hydrogen peroxide | cupric sulfide | water | mixed sulfur | copper(II) chloride IUPAC name | hydrogen chloride | hydrogen peroxide | | water | sulfur | dichlorocopper

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