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SO2 + NaHCO3 = CO2 + NaHSO3

Input interpretation

SO_2 sulfur dioxide + NaHCO_3 sodium bicarbonate ⟶ CO_2 carbon dioxide + NaHSO_3 sodium bisulfite
SO_2 sulfur dioxide + NaHCO_3 sodium bicarbonate ⟶ CO_2 carbon dioxide + NaHSO_3 sodium bisulfite

Balanced equation

Balance the chemical equation algebraically: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SO_2 + c_2 NaHCO_3 ⟶ c_3 CO_2 + c_4 NaHSO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S, C, H and Na: O: | 2 c_1 + 3 c_2 = 2 c_3 + 3 c_4 S: | c_1 = c_4 C: | c_2 = c_3 H: | c_2 = c_4 Na: | c_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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3
Balance the chemical equation algebraically: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SO_2 + c_2 NaHCO_3 ⟶ c_3 CO_2 + c_4 NaHSO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for O, S, C, H and Na: O: | 2 c_1 + 3 c_2 = 2 c_3 + 3 c_4 S: | c_1 = c_4 C: | c_2 = c_3 H: | c_2 = c_4 Na: | c_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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3

Structures

+ ⟶ +
+ ⟶ +

Names

sulfur dioxide + sodium bicarbonate ⟶ carbon dioxide + sodium bisulfite
sulfur dioxide + sodium bicarbonate ⟶ carbon dioxide + sodium bisulfite

Equilibrium constant

Construct the equilibrium constant, K, expression for: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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 SO_2 | 1 | -1 NaHCO_3 | 1 | -1 CO_2 | 1 | 1 NaHSO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SO_2 | 1 | -1 | ([SO2])^(-1) NaHCO_3 | 1 | -1 | ([NaHCO3])^(-1) CO_2 | 1 | 1 | [CO2] NaHSO_3 | 1 | 1 | [NaHSO3] 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 = ([SO2])^(-1) ([NaHCO3])^(-1) [CO2] [NaHSO3] = ([CO2] [NaHSO3])/([SO2] [NaHCO3])
Construct the equilibrium constant, K, expression for: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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 SO_2 | 1 | -1 NaHCO_3 | 1 | -1 CO_2 | 1 | 1 NaHSO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SO_2 | 1 | -1 | ([SO2])^(-1) NaHCO_3 | 1 | -1 | ([NaHCO3])^(-1) CO_2 | 1 | 1 | [CO2] NaHSO_3 | 1 | 1 | [NaHSO3] 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 = ([SO2])^(-1) ([NaHCO3])^(-1) [CO2] [NaHSO3] = ([CO2] [NaHSO3])/([SO2] [NaHCO3])

Rate of reaction

Construct the rate of reaction expression for: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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 SO_2 | 1 | -1 NaHCO_3 | 1 | -1 CO_2 | 1 | 1 NaHSO_3 | 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 SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) NaHCO_3 | 1 | -1 | -(Δ[NaHCO3])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) NaHSO_3 | 1 | 1 | (Δ[NaHSO3])/(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[SO2])/(Δt) = -(Δ[NaHCO3])/(Δt) = (Δ[CO2])/(Δt) = (Δ[NaHSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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: SO_2 + NaHCO_3 ⟶ CO_2 + NaHSO_3 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 SO_2 | 1 | -1 NaHCO_3 | 1 | -1 CO_2 | 1 | 1 NaHSO_3 | 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 SO_2 | 1 | -1 | -(Δ[SO2])/(Δt) NaHCO_3 | 1 | -1 | -(Δ[NaHCO3])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) NaHSO_3 | 1 | 1 | (Δ[NaHSO3])/(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[SO2])/(Δt) = -(Δ[NaHCO3])/(Δt) = (Δ[CO2])/(Δt) = (Δ[NaHSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfur dioxide | sodium bicarbonate | carbon dioxide | sodium bisulfite formula | SO_2 | NaHCO_3 | CO_2 | NaHSO_3 Hill formula | O_2S | CHNaO_3 | CO_2 | HNaO_3S name | sulfur dioxide | sodium bicarbonate | carbon dioxide | sodium bisulfite IUPAC name | sulfur dioxide | sodium hydrogen carbonate | carbon dioxide |
| sulfur dioxide | sodium bicarbonate | carbon dioxide | sodium bisulfite formula | SO_2 | NaHCO_3 | CO_2 | NaHSO_3 Hill formula | O_2S | CHNaO_3 | CO_2 | HNaO_3S name | sulfur dioxide | sodium bicarbonate | carbon dioxide | sodium bisulfite IUPAC name | sulfur dioxide | sodium hydrogen carbonate | carbon dioxide |

Substance properties

| sulfur dioxide | sodium bicarbonate | carbon dioxide | sodium bisulfite molar mass | 64.06 g/mol | 84.006 g/mol | 44.009 g/mol | 104.1 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -73 °C | 270 °C | -56.56 °C (at triple point) | 150 °C boiling point | -10 °C | | -78.5 °C (at sublimation point) | density | 0.002619 g/cm^3 (at 25 °C) | 2.16 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 1.36 g/cm^3 solubility in water | | soluble | | surface tension | 0.02859 N/m | | | dynamic viscosity | 1.282×10^-5 Pa s (at 25 °C) | | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless |
| sulfur dioxide | sodium bicarbonate | carbon dioxide | sodium bisulfite molar mass | 64.06 g/mol | 84.006 g/mol | 44.009 g/mol | 104.1 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -73 °C | 270 °C | -56.56 °C (at triple point) | 150 °C boiling point | -10 °C | | -78.5 °C (at sublimation point) | density | 0.002619 g/cm^3 (at 25 °C) | 2.16 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 1.36 g/cm^3 solubility in water | | soluble | | surface tension | 0.02859 N/m | | | dynamic viscosity | 1.282×10^-5 Pa s (at 25 °C) | | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless |

Units

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