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CuO + C2H5OH = H2O + Cu + H3CCOOH

Input interpretation

CuO cupric oxide + CH_3CH_2OH ethanol ⟶ H_2O water + Cu copper + CH_3CO_2H acetic acid
CuO cupric oxide + CH_3CH_2OH ethanol ⟶ H_2O water + Cu copper + CH_3CO_2H acetic acid

Balanced equation

Balance the chemical equation algebraically: CuO + CH_3CH_2OH ⟶ H_2O + Cu + CH_3CO_2H Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 CH_3CH_2OH ⟶ c_3 H_2O + c_4 Cu + c_5 CH_3CO_2H Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, C and H: Cu: | c_1 = c_4 O: | c_1 + c_2 = c_3 + 2 c_5 C: | 2 c_2 = 2 c_5 H: | 6 c_2 = 2 c_3 + 4 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 CuO + CH_3CH_2OH ⟶ H_2O + 2 Cu + CH_3CO_2H
Balance the chemical equation algebraically: CuO + CH_3CH_2OH ⟶ H_2O + Cu + CH_3CO_2H Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 CH_3CH_2OH ⟶ c_3 H_2O + c_4 Cu + c_5 CH_3CO_2H Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, C and H: Cu: | c_1 = c_4 O: | c_1 + c_2 = c_3 + 2 c_5 C: | 2 c_2 = 2 c_5 H: | 6 c_2 = 2 c_3 + 4 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 CuO + CH_3CH_2OH ⟶ H_2O + 2 Cu + CH_3CO_2H

Structures

+ ⟶ + +
+ ⟶ + +

Names

cupric oxide + ethanol ⟶ water + copper + acetic acid
cupric oxide + ethanol ⟶ water + copper + acetic acid

Reaction thermodynamics

Entropy

| cupric oxide | ethanol | water | copper | acetic acid molecular entropy | 43 J/(mol K) | 160.7 J/(mol K) | 69.91 J/(mol K) | 33 J/(mol K) | 160 J/(mol K) total entropy | 86 J/(mol K) | 160.7 J/(mol K) | 69.91 J/(mol K) | 66 J/(mol K) | 160 J/(mol K) | S_initial = 246.7 J/(mol K) | | S_final = 295.9 J/(mol K) | | ΔS_rxn^0 | 295.9 J/(mol K) - 246.7 J/(mol K) = 49.21 J/(mol K) (endoentropic) | | | |
| cupric oxide | ethanol | water | copper | acetic acid molecular entropy | 43 J/(mol K) | 160.7 J/(mol K) | 69.91 J/(mol K) | 33 J/(mol K) | 160 J/(mol K) total entropy | 86 J/(mol K) | 160.7 J/(mol K) | 69.91 J/(mol K) | 66 J/(mol K) | 160 J/(mol K) | S_initial = 246.7 J/(mol K) | | S_final = 295.9 J/(mol K) | | ΔS_rxn^0 | 295.9 J/(mol K) - 246.7 J/(mol K) = 49.21 J/(mol K) (endoentropic) | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: CuO + CH_3CH_2OH ⟶ H_2O + Cu + CH_3CO_2H 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 CuO + CH_3CH_2OH ⟶ H_2O + 2 Cu + CH_3CO_2H 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 CuO | 2 | -2 CH_3CH_2OH | 1 | -1 H_2O | 1 | 1 Cu | 2 | 2 CH_3CO_2H | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 2 | -2 | ([CuO])^(-2) CH_3CH_2OH | 1 | -1 | ([CH3CH2OH])^(-1) H_2O | 1 | 1 | [H2O] Cu | 2 | 2 | ([Cu])^2 CH_3CO_2H | 1 | 1 | [CH3CO2H] 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 = ([CuO])^(-2) ([CH3CH2OH])^(-1) [H2O] ([Cu])^2 [CH3CO2H] = ([H2O] ([Cu])^2 [CH3CO2H])/(([CuO])^2 [CH3CH2OH])
Construct the equilibrium constant, K, expression for: CuO + CH_3CH_2OH ⟶ H_2O + Cu + CH_3CO_2H 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 CuO + CH_3CH_2OH ⟶ H_2O + 2 Cu + CH_3CO_2H 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 CuO | 2 | -2 CH_3CH_2OH | 1 | -1 H_2O | 1 | 1 Cu | 2 | 2 CH_3CO_2H | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 2 | -2 | ([CuO])^(-2) CH_3CH_2OH | 1 | -1 | ([CH3CH2OH])^(-1) H_2O | 1 | 1 | [H2O] Cu | 2 | 2 | ([Cu])^2 CH_3CO_2H | 1 | 1 | [CH3CO2H] 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 = ([CuO])^(-2) ([CH3CH2OH])^(-1) [H2O] ([Cu])^2 [CH3CO2H] = ([H2O] ([Cu])^2 [CH3CO2H])/(([CuO])^2 [CH3CH2OH])

Rate of reaction

Construct the rate of reaction expression for: CuO + CH_3CH_2OH ⟶ H_2O + Cu + CH_3CO_2H 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 CuO + CH_3CH_2OH ⟶ H_2O + 2 Cu + CH_3CO_2H 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 CuO | 2 | -2 CH_3CH_2OH | 1 | -1 H_2O | 1 | 1 Cu | 2 | 2 CH_3CO_2H | 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 CuO | 2 | -2 | -1/2 (Δ[CuO])/(Δt) CH_3CH_2OH | 1 | -1 | -(Δ[CH3CH2OH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cu | 2 | 2 | 1/2 (Δ[Cu])/(Δt) CH_3CO_2H | 1 | 1 | (Δ[CH3CO2H])/(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[CuO])/(Δt) = -(Δ[CH3CH2OH])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[Cu])/(Δt) = (Δ[CH3CO2H])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CuO + CH_3CH_2OH ⟶ H_2O + Cu + CH_3CO_2H 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 CuO + CH_3CH_2OH ⟶ H_2O + 2 Cu + CH_3CO_2H 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 CuO | 2 | -2 CH_3CH_2OH | 1 | -1 H_2O | 1 | 1 Cu | 2 | 2 CH_3CO_2H | 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 CuO | 2 | -2 | -1/2 (Δ[CuO])/(Δt) CH_3CH_2OH | 1 | -1 | -(Δ[CH3CH2OH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cu | 2 | 2 | 1/2 (Δ[Cu])/(Δt) CH_3CO_2H | 1 | 1 | (Δ[CH3CO2H])/(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[CuO])/(Δt) = -(Δ[CH3CH2OH])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[Cu])/(Δt) = (Δ[CH3CO2H])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| cupric oxide | ethanol | water | copper | acetic acid formula | CuO | CH_3CH_2OH | H_2O | Cu | CH_3CO_2H Hill formula | CuO | C_2H_6O | H_2O | Cu | C_2H_4O_2 name | cupric oxide | ethanol | water | copper | acetic acid
| cupric oxide | ethanol | water | copper | acetic acid formula | CuO | CH_3CH_2OH | H_2O | Cu | CH_3CO_2H Hill formula | CuO | C_2H_6O | H_2O | Cu | C_2H_4O_2 name | cupric oxide | ethanol | water | copper | acetic acid

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