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Na + CH3COOH = H2 + CH3COONa

Input interpretation

Na sodium + CH_3CO_2H acetic acid ⟶ H_2 hydrogen + CH_3COONa sodium acetate
Na sodium + CH_3CO_2H acetic acid ⟶ H_2 hydrogen + CH_3COONa sodium acetate

Balanced equation

Balance the chemical equation algebraically: Na + CH_3CO_2H ⟶ H_2 + CH_3COONa Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na + c_2 CH_3CO_2H ⟶ c_3 H_2 + c_4 CH_3COONa Set the number of atoms in the reactants equal to the number of atoms in the products for Na, C, H and O: Na: | c_1 = c_4 C: | 2 c_2 = 2 c_4 H: | 4 c_2 = 2 c_3 + 3 c_4 O: | 2 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Na + 2 CH_3CO_2H ⟶ H_2 + 2 CH_3COONa
Balance the chemical equation algebraically: Na + CH_3CO_2H ⟶ H_2 + CH_3COONa Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Na + c_2 CH_3CO_2H ⟶ c_3 H_2 + c_4 CH_3COONa Set the number of atoms in the reactants equal to the number of atoms in the products for Na, C, H and O: Na: | c_1 = c_4 C: | 2 c_2 = 2 c_4 H: | 4 c_2 = 2 c_3 + 3 c_4 O: | 2 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Na + 2 CH_3CO_2H ⟶ H_2 + 2 CH_3COONa

Structures

+ ⟶ +
+ ⟶ +

Names

sodium + acetic acid ⟶ hydrogen + sodium acetate
sodium + acetic acid ⟶ hydrogen + sodium acetate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Na + CH_3CO_2H ⟶ H_2 + CH_3COONa 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 Na + 2 CH_3CO_2H ⟶ H_2 + 2 CH_3COONa 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 Na | 2 | -2 CH_3CO_2H | 2 | -2 H_2 | 1 | 1 CH_3COONa | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na | 2 | -2 | ([Na])^(-2) CH_3CO_2H | 2 | -2 | ([CH3CO2H])^(-2) H_2 | 1 | 1 | [H2] CH_3COONa | 2 | 2 | ([CH3COONa])^2 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 = ([Na])^(-2) ([CH3CO2H])^(-2) [H2] ([CH3COONa])^2 = ([H2] ([CH3COONa])^2)/(([Na])^2 ([CH3CO2H])^2)
Construct the equilibrium constant, K, expression for: Na + CH_3CO_2H ⟶ H_2 + CH_3COONa 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 Na + 2 CH_3CO_2H ⟶ H_2 + 2 CH_3COONa 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 Na | 2 | -2 CH_3CO_2H | 2 | -2 H_2 | 1 | 1 CH_3COONa | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Na | 2 | -2 | ([Na])^(-2) CH_3CO_2H | 2 | -2 | ([CH3CO2H])^(-2) H_2 | 1 | 1 | [H2] CH_3COONa | 2 | 2 | ([CH3COONa])^2 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 = ([Na])^(-2) ([CH3CO2H])^(-2) [H2] ([CH3COONa])^2 = ([H2] ([CH3COONa])^2)/(([Na])^2 ([CH3CO2H])^2)

Rate of reaction

Construct the rate of reaction expression for: Na + CH_3CO_2H ⟶ H_2 + CH_3COONa 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 Na + 2 CH_3CO_2H ⟶ H_2 + 2 CH_3COONa 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 Na | 2 | -2 CH_3CO_2H | 2 | -2 H_2 | 1 | 1 CH_3COONa | 2 | 2 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 Na | 2 | -2 | -1/2 (Δ[Na])/(Δt) CH_3CO_2H | 2 | -2 | -1/2 (Δ[CH3CO2H])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) CH_3COONa | 2 | 2 | 1/2 (Δ[CH3COONa])/(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[Na])/(Δt) = -1/2 (Δ[CH3CO2H])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[CH3COONa])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Na + CH_3CO_2H ⟶ H_2 + CH_3COONa 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 Na + 2 CH_3CO_2H ⟶ H_2 + 2 CH_3COONa 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 Na | 2 | -2 CH_3CO_2H | 2 | -2 H_2 | 1 | 1 CH_3COONa | 2 | 2 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 Na | 2 | -2 | -1/2 (Δ[Na])/(Δt) CH_3CO_2H | 2 | -2 | -1/2 (Δ[CH3CO2H])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) CH_3COONa | 2 | 2 | 1/2 (Δ[CH3COONa])/(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[Na])/(Δt) = -1/2 (Δ[CH3CO2H])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[CH3COONa])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium | acetic acid | hydrogen | sodium acetate formula | Na | CH_3CO_2H | H_2 | CH_3COONa Hill formula | Na | C_2H_4O_2 | H_2 | C_2H_3NaO_2 name | sodium | acetic acid | hydrogen | sodium acetate IUPAC name | sodium | acetic acid | molecular hydrogen | sodium acetate
| sodium | acetic acid | hydrogen | sodium acetate formula | Na | CH_3CO_2H | H_2 | CH_3COONa Hill formula | Na | C_2H_4O_2 | H_2 | C_2H_3NaO_2 name | sodium | acetic acid | hydrogen | sodium acetate IUPAC name | sodium | acetic acid | molecular hydrogen | sodium acetate

Substance properties

| sodium | acetic acid | hydrogen | sodium acetate molar mass | 22.98976928 g/mol | 60.052 g/mol | 2.016 g/mol | 82.034 g/mol phase | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 97.8 °C | 16.2 °C | -259.2 °C | 300 °C boiling point | 883 °C | 117.5 °C | -252.8 °C | 881.4 °C density | 0.968 g/cm^3 | 1.049 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.528 g/cm^3 solubility in water | decomposes | miscible | | soluble surface tension | | 0.0288 N/m | | dynamic viscosity | 1.413×10^-5 Pa s (at 527 °C) | 0.001056 Pa s (at 25 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | | vinegar-like | odorless | odorless
| sodium | acetic acid | hydrogen | sodium acetate molar mass | 22.98976928 g/mol | 60.052 g/mol | 2.016 g/mol | 82.034 g/mol phase | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 97.8 °C | 16.2 °C | -259.2 °C | 300 °C boiling point | 883 °C | 117.5 °C | -252.8 °C | 881.4 °C density | 0.968 g/cm^3 | 1.049 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.528 g/cm^3 solubility in water | decomposes | miscible | | soluble surface tension | | 0.0288 N/m | | dynamic viscosity | 1.413×10^-5 Pa s (at 527 °C) | 0.001056 Pa s (at 25 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | | vinegar-like | odorless | odorless

Units

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