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H2SO4 + (NH4)2CO3 = H2O + CO2 + (NH4)2SO4

Input interpretation

H_2SO_4 sulfuric acid + (NH_4)_2CO_3 ammonium carbonate ⟶ H_2O water + CO_2 carbon dioxide + (NH_4)_2SO_4 ammonium sulfate
H_2SO_4 sulfuric acid + (NH_4)_2CO_3 ammonium carbonate ⟶ H_2O water + CO_2 carbon dioxide + (NH_4)_2SO_4 ammonium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 (NH_4)_2CO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 (NH_4)_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, C and N: H: | 2 c_1 + 8 c_2 = 2 c_3 + 8 c_5 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 4 c_5 S: | c_1 = c_5 C: | c_2 = c_4 N: | 2 c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4
Balance the chemical equation algebraically: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 (NH_4)_2CO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 (NH_4)_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, C and N: H: | 2 c_1 + 8 c_2 = 2 c_3 + 8 c_5 O: | 4 c_1 + 3 c_2 = c_3 + 2 c_4 + 4 c_5 S: | c_1 = c_5 C: | c_2 = c_4 N: | 2 c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4

Structures

+ ⟶ + +
+ ⟶ + +

Names

sulfuric acid + ammonium carbonate ⟶ water + carbon dioxide + ammonium sulfate
sulfuric acid + ammonium carbonate ⟶ water + carbon dioxide + ammonium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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 H_2SO_4 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 (NH_4)_2SO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) (NH_4)_2CO_3 | 1 | -1 | ([(NH4)2CO3])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] (NH_4)_2SO_4 | 1 | 1 | [(NH4)2SO4] 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 = ([H2SO4])^(-1) ([(NH4)2CO3])^(-1) [H2O] [CO2] [(NH4)2SO4] = ([H2O] [CO2] [(NH4)2SO4])/([H2SO4] [(NH4)2CO3])
Construct the equilibrium constant, K, expression for: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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 H_2SO_4 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 (NH_4)_2SO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) (NH_4)_2CO_3 | 1 | -1 | ([(NH4)2CO3])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] (NH_4)_2SO_4 | 1 | 1 | [(NH4)2SO4] 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 = ([H2SO4])^(-1) ([(NH4)2CO3])^(-1) [H2O] [CO2] [(NH4)2SO4] = ([H2O] [CO2] [(NH4)2SO4])/([H2SO4] [(NH4)2CO3])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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 H_2SO_4 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 (NH_4)_2SO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) (NH_4)_2CO_3 | 1 | -1 | -(Δ[(NH4)2CO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) (NH_4)_2SO_4 | 1 | 1 | (Δ[(NH4)2SO4])/(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[H2SO4])/(Δt) = -(Δ[(NH4)2CO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[(NH4)2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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: H_2SO_4 + (NH_4)_2CO_3 ⟶ H_2O + CO_2 + (NH_4)_2SO_4 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 H_2SO_4 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 (NH_4)_2SO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) (NH_4)_2CO_3 | 1 | -1 | -(Δ[(NH4)2CO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) (NH_4)_2SO_4 | 1 | 1 | (Δ[(NH4)2SO4])/(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[H2SO4])/(Δt) = -(Δ[(NH4)2CO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[(NH4)2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | ammonium carbonate | water | carbon dioxide | ammonium sulfate formula | H_2SO_4 | (NH_4)_2CO_3 | H_2O | CO_2 | (NH_4)_2SO_4 Hill formula | H_2O_4S | CH_8N_2O_3 | H_2O | CO_2 | H_8N_2O_4S name | sulfuric acid | ammonium carbonate | water | carbon dioxide | ammonium sulfate
| sulfuric acid | ammonium carbonate | water | carbon dioxide | ammonium sulfate formula | H_2SO_4 | (NH_4)_2CO_3 | H_2O | CO_2 | (NH_4)_2SO_4 Hill formula | H_2O_4S | CH_8N_2O_3 | H_2O | CO_2 | H_8N_2O_4S name | sulfuric acid | ammonium carbonate | water | carbon dioxide | ammonium sulfate

Substance properties

| sulfuric acid | ammonium carbonate | water | carbon dioxide | ammonium sulfate molar mass | 98.07 g/mol | 96.09 g/mol | 18.015 g/mol | 44.009 g/mol | 132.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 10.371 °C | 58 °C | 0 °C | -56.56 °C (at triple point) | 280 °C boiling point | 279.6 °C | | 99.9839 °C | -78.5 °C (at sublimation point) | density | 1.8305 g/cm^3 | 1.5 g/cm^3 | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 1.77 g/cm^3 solubility in water | very soluble | soluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless | odorless | odorless
| sulfuric acid | ammonium carbonate | water | carbon dioxide | ammonium sulfate molar mass | 98.07 g/mol | 96.09 g/mol | 18.015 g/mol | 44.009 g/mol | 132.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 10.371 °C | 58 °C | 0 °C | -56.56 °C (at triple point) | 280 °C boiling point | 279.6 °C | | 99.9839 °C | -78.5 °C (at sublimation point) | density | 1.8305 g/cm^3 | 1.5 g/cm^3 | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 1.77 g/cm^3 solubility in water | very soluble | soluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless | odorless | odorless

Units

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