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HCl + Cu + H2O2 = H2O + CuCl2

Input interpretation

HCl hydrogen chloride + Cu copper + H_2O_2 hydrogen peroxide ⟶ H_2O water + CuCl_2 copper(II) chloride
HCl hydrogen chloride + Cu copper + H_2O_2 hydrogen peroxide ⟶ H_2O water + CuCl_2 copper(II) chloride

Balanced equation

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

Structures

+ + ⟶ +
+ + ⟶ +

Names

hydrogen chloride + copper + hydrogen peroxide ⟶ water + copper(II) chloride
hydrogen chloride + copper + hydrogen peroxide ⟶ water + copper(II) chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Cu + H_2O_2 ⟶ H_2O + 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 + Cu + H_2O_2 ⟶ 2 H_2O + 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 Cu | 1 | -1 H_2O_2 | 1 | -1 H_2O | 2 | 2 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) Cu | 1 | -1 | ([Cu])^(-1) H_2O_2 | 1 | -1 | ([H2O2])^(-1) H_2O | 2 | 2 | ([H2O])^2 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) ([Cu])^(-1) ([H2O2])^(-1) ([H2O])^2 [CuCl2] = (([H2O])^2 [CuCl2])/(([HCl])^2 [Cu] [H2O2])
Construct the equilibrium constant, K, expression for: HCl + Cu + H_2O_2 ⟶ H_2O + 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 + Cu + H_2O_2 ⟶ 2 H_2O + 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 Cu | 1 | -1 H_2O_2 | 1 | -1 H_2O | 2 | 2 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) Cu | 1 | -1 | ([Cu])^(-1) H_2O_2 | 1 | -1 | ([H2O2])^(-1) H_2O | 2 | 2 | ([H2O])^2 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) ([Cu])^(-1) ([H2O2])^(-1) ([H2O])^2 [CuCl2] = (([H2O])^2 [CuCl2])/(([HCl])^2 [Cu] [H2O2])

Rate of reaction

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

Chemical names and formulas

| hydrogen chloride | copper | hydrogen peroxide | water | copper(II) chloride formula | HCl | Cu | H_2O_2 | H_2O | CuCl_2 Hill formula | ClH | Cu | H_2O_2 | H_2O | Cl_2Cu name | hydrogen chloride | copper | hydrogen peroxide | water | copper(II) chloride IUPAC name | hydrogen chloride | copper | hydrogen peroxide | water | dichlorocopper
| hydrogen chloride | copper | hydrogen peroxide | water | copper(II) chloride formula | HCl | Cu | H_2O_2 | H_2O | CuCl_2 Hill formula | ClH | Cu | H_2O_2 | H_2O | Cl_2Cu name | hydrogen chloride | copper | hydrogen peroxide | water | copper(II) chloride IUPAC name | hydrogen chloride | copper | hydrogen peroxide | water | dichlorocopper

Substance properties

| hydrogen chloride | copper | hydrogen peroxide | water | copper(II) chloride molar mass | 36.46 g/mol | 63.546 g/mol | 34.014 g/mol | 18.015 g/mol | 134.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 1083 °C | -0.43 °C | 0 °C | 620 °C boiling point | -85 °C | 2567 °C | 150.2 °C | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | 8.96 g/cm^3 | 1.44 g/cm^3 | 1 g/cm^3 | 3.386 g/cm^3 solubility in water | miscible | insoluble | miscible | | surface tension | | | 0.0804 N/m | 0.0728 N/m | dynamic viscosity | | | 0.001249 Pa s (at 20 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless | | odorless |
| hydrogen chloride | copper | hydrogen peroxide | water | copper(II) chloride molar mass | 36.46 g/mol | 63.546 g/mol | 34.014 g/mol | 18.015 g/mol | 134.4 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 1083 °C | -0.43 °C | 0 °C | 620 °C boiling point | -85 °C | 2567 °C | 150.2 °C | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | 8.96 g/cm^3 | 1.44 g/cm^3 | 1 g/cm^3 | 3.386 g/cm^3 solubility in water | miscible | insoluble | miscible | | surface tension | | | 0.0804 N/m | 0.0728 N/m | dynamic viscosity | | | 0.001249 Pa s (at 20 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless | | odorless |

Units

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