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CuSO4 + HCN = H2SO4 + Cu(CN)2

Input interpretation

CuSO_4 copper(II) sulfate + HCN hydrogen cyanide ⟶ H_2SO_4 sulfuric acid + C_2CuN_2 cupric cyanide
CuSO_4 copper(II) sulfate + HCN hydrogen cyanide ⟶ H_2SO_4 sulfuric acid + C_2CuN_2 cupric cyanide

Balanced equation

Balance the chemical equation algebraically: CuSO_4 + HCN ⟶ H_2SO_4 + C_2CuN_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuSO_4 + c_2 HCN ⟶ c_3 H_2SO_4 + c_4 C_2CuN_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, S, C, H and N: Cu: | c_1 = c_4 O: | 4 c_1 = 4 c_3 S: | c_1 = c_3 C: | c_2 = 2 c_4 H: | c_2 = 2 c_3 N: | c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuSO_4 + 2 HCN ⟶ H_2SO_4 + C_2CuN_2
Balance the chemical equation algebraically: CuSO_4 + HCN ⟶ H_2SO_4 + C_2CuN_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuSO_4 + c_2 HCN ⟶ c_3 H_2SO_4 + c_4 C_2CuN_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, S, C, H and N: Cu: | c_1 = c_4 O: | 4 c_1 = 4 c_3 S: | c_1 = c_3 C: | c_2 = 2 c_4 H: | c_2 = 2 c_3 N: | c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuSO_4 + 2 HCN ⟶ H_2SO_4 + C_2CuN_2

Structures

+ ⟶ +
+ ⟶ +

Names

copper(II) sulfate + hydrogen cyanide ⟶ sulfuric acid + cupric cyanide
copper(II) sulfate + hydrogen cyanide ⟶ sulfuric acid + cupric cyanide

Equilibrium constant

Construct the equilibrium constant, K, expression for: CuSO_4 + HCN ⟶ H_2SO_4 + C_2CuN_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: CuSO_4 + 2 HCN ⟶ H_2SO_4 + C_2CuN_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 CuSO_4 | 1 | -1 HCN | 2 | -2 H_2SO_4 | 1 | 1 C_2CuN_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuSO_4 | 1 | -1 | ([CuSO4])^(-1) HCN | 2 | -2 | ([HCN])^(-2) H_2SO_4 | 1 | 1 | [H2SO4] C_2CuN_2 | 1 | 1 | [C2CuN2] 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 = ([CuSO4])^(-1) ([HCN])^(-2) [H2SO4] [C2CuN2] = ([H2SO4] [C2CuN2])/([CuSO4] ([HCN])^2)
Construct the equilibrium constant, K, expression for: CuSO_4 + HCN ⟶ H_2SO_4 + C_2CuN_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: CuSO_4 + 2 HCN ⟶ H_2SO_4 + C_2CuN_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 CuSO_4 | 1 | -1 HCN | 2 | -2 H_2SO_4 | 1 | 1 C_2CuN_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuSO_4 | 1 | -1 | ([CuSO4])^(-1) HCN | 2 | -2 | ([HCN])^(-2) H_2SO_4 | 1 | 1 | [H2SO4] C_2CuN_2 | 1 | 1 | [C2CuN2] 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 = ([CuSO4])^(-1) ([HCN])^(-2) [H2SO4] [C2CuN2] = ([H2SO4] [C2CuN2])/([CuSO4] ([HCN])^2)

Rate of reaction

Construct the rate of reaction expression for: CuSO_4 + HCN ⟶ H_2SO_4 + C_2CuN_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: CuSO_4 + 2 HCN ⟶ H_2SO_4 + C_2CuN_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 CuSO_4 | 1 | -1 HCN | 2 | -2 H_2SO_4 | 1 | 1 C_2CuN_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 CuSO_4 | 1 | -1 | -(Δ[CuSO4])/(Δt) HCN | 2 | -2 | -1/2 (Δ[HCN])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) C_2CuN_2 | 1 | 1 | (Δ[C2CuN2])/(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 = -(Δ[CuSO4])/(Δt) = -1/2 (Δ[HCN])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[C2CuN2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CuSO_4 + HCN ⟶ H_2SO_4 + C_2CuN_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: CuSO_4 + 2 HCN ⟶ H_2SO_4 + C_2CuN_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 CuSO_4 | 1 | -1 HCN | 2 | -2 H_2SO_4 | 1 | 1 C_2CuN_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 CuSO_4 | 1 | -1 | -(Δ[CuSO4])/(Δt) HCN | 2 | -2 | -1/2 (Δ[HCN])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) C_2CuN_2 | 1 | 1 | (Δ[C2CuN2])/(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 = -(Δ[CuSO4])/(Δt) = -1/2 (Δ[HCN])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[C2CuN2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| copper(II) sulfate | hydrogen cyanide | sulfuric acid | cupric cyanide formula | CuSO_4 | HCN | H_2SO_4 | C_2CuN_2 Hill formula | CuO_4S | CHN | H_2O_4S | C_2CuN_2 name | copper(II) sulfate | hydrogen cyanide | sulfuric acid | cupric cyanide IUPAC name | copper sulfate | formonitrile | sulfuric acid | copper dicyanide
| copper(II) sulfate | hydrogen cyanide | sulfuric acid | cupric cyanide formula | CuSO_4 | HCN | H_2SO_4 | C_2CuN_2 Hill formula | CuO_4S | CHN | H_2O_4S | C_2CuN_2 name | copper(II) sulfate | hydrogen cyanide | sulfuric acid | cupric cyanide IUPAC name | copper sulfate | formonitrile | sulfuric acid | copper dicyanide

Substance properties

| copper(II) sulfate | hydrogen cyanide | sulfuric acid | cupric cyanide molar mass | 159.6 g/mol | 27.026 g/mol | 98.07 g/mol | 115.58 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | melting point | 200 °C | -13.4 °C | 10.371 °C | boiling point | | 25.6 °C | 279.6 °C | density | 3.603 g/cm^3 | 0.697 g/cm^3 | 1.8305 g/cm^3 | solubility in water | | miscible | very soluble | surface tension | | 0.0172 N/m | 0.0735 N/m | dynamic viscosity | | 1.83×10^-4 Pa s (at 25 °C) | 0.021 Pa s (at 25 °C) | odor | | | odorless |
| copper(II) sulfate | hydrogen cyanide | sulfuric acid | cupric cyanide molar mass | 159.6 g/mol | 27.026 g/mol | 98.07 g/mol | 115.58 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | melting point | 200 °C | -13.4 °C | 10.371 °C | boiling point | | 25.6 °C | 279.6 °C | density | 3.603 g/cm^3 | 0.697 g/cm^3 | 1.8305 g/cm^3 | solubility in water | | miscible | very soluble | surface tension | | 0.0172 N/m | 0.0735 N/m | dynamic viscosity | | 1.83×10^-4 Pa s (at 25 °C) | 0.021 Pa s (at 25 °C) | odor | | | odorless |

Units

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