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HNO3 + Al2(CO3)3 = H2O + CO2 + Al(NO3)3

Input interpretation

HNO_3 nitric acid + Al2(CO3)3 ⟶ H_2O water + CO_2 carbon dioxide + Al(NO_3)_3 aluminum nitrate
HNO_3 nitric acid + Al2(CO3)3 ⟶ H_2O water + CO_2 carbon dioxide + Al(NO_3)_3 aluminum nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Al2(CO3)3 ⟶ H_2O + CO_2 + Al(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Al2(CO3)3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 Al(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Al and C: H: | c_1 = 2 c_3 N: | c_1 = 3 c_5 O: | 3 c_1 + 9 c_2 = c_3 + 2 c_4 + 9 c_5 Al: | 2 c_2 = c_5 C: | 3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 1 c_3 = 3 c_4 = 3 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HNO_3 + Al2(CO3)3 ⟶ 3 H_2O + 3 CO_2 + 2 Al(NO_3)_3
Balance the chemical equation algebraically: HNO_3 + Al2(CO3)3 ⟶ H_2O + CO_2 + Al(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Al2(CO3)3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 Al(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Al and C: H: | c_1 = 2 c_3 N: | c_1 = 3 c_5 O: | 3 c_1 + 9 c_2 = c_3 + 2 c_4 + 9 c_5 Al: | 2 c_2 = c_5 C: | 3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 1 c_3 = 3 c_4 = 3 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HNO_3 + Al2(CO3)3 ⟶ 3 H_2O + 3 CO_2 + 2 Al(NO_3)_3

Structures

+ Al2(CO3)3 ⟶ + +
+ Al2(CO3)3 ⟶ + +

Names

nitric acid + Al2(CO3)3 ⟶ water + carbon dioxide + aluminum nitrate
nitric acid + Al2(CO3)3 ⟶ water + carbon dioxide + aluminum nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Al2(CO3)3 ⟶ H_2O + CO_2 + Al(NO_3)_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: 6 HNO_3 + Al2(CO3)3 ⟶ 3 H_2O + 3 CO_2 + 2 Al(NO_3)_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 HNO_3 | 6 | -6 Al2(CO3)3 | 1 | -1 H_2O | 3 | 3 CO_2 | 3 | 3 Al(NO_3)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 6 | -6 | ([HNO3])^(-6) Al2(CO3)3 | 1 | -1 | ([Al2(CO3)3])^(-1) H_2O | 3 | 3 | ([H2O])^3 CO_2 | 3 | 3 | ([CO2])^3 Al(NO_3)_3 | 2 | 2 | ([Al(NO3)3])^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 = ([HNO3])^(-6) ([Al2(CO3)3])^(-1) ([H2O])^3 ([CO2])^3 ([Al(NO3)3])^2 = (([H2O])^3 ([CO2])^3 ([Al(NO3)3])^2)/(([HNO3])^6 [Al2(CO3)3])
Construct the equilibrium constant, K, expression for: HNO_3 + Al2(CO3)3 ⟶ H_2O + CO_2 + Al(NO_3)_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: 6 HNO_3 + Al2(CO3)3 ⟶ 3 H_2O + 3 CO_2 + 2 Al(NO_3)_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 HNO_3 | 6 | -6 Al2(CO3)3 | 1 | -1 H_2O | 3 | 3 CO_2 | 3 | 3 Al(NO_3)_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 6 | -6 | ([HNO3])^(-6) Al2(CO3)3 | 1 | -1 | ([Al2(CO3)3])^(-1) H_2O | 3 | 3 | ([H2O])^3 CO_2 | 3 | 3 | ([CO2])^3 Al(NO_3)_3 | 2 | 2 | ([Al(NO3)3])^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 = ([HNO3])^(-6) ([Al2(CO3)3])^(-1) ([H2O])^3 ([CO2])^3 ([Al(NO3)3])^2 = (([H2O])^3 ([CO2])^3 ([Al(NO3)3])^2)/(([HNO3])^6 [Al2(CO3)3])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Al2(CO3)3 ⟶ H_2O + CO_2 + Al(NO_3)_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: 6 HNO_3 + Al2(CO3)3 ⟶ 3 H_2O + 3 CO_2 + 2 Al(NO_3)_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 HNO_3 | 6 | -6 Al2(CO3)3 | 1 | -1 H_2O | 3 | 3 CO_2 | 3 | 3 Al(NO_3)_3 | 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 HNO_3 | 6 | -6 | -1/6 (Δ[HNO3])/(Δt) Al2(CO3)3 | 1 | -1 | -(Δ[Al2(CO3)3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) CO_2 | 3 | 3 | 1/3 (Δ[CO2])/(Δt) Al(NO_3)_3 | 2 | 2 | 1/2 (Δ[Al(NO3)3])/(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 = -1/6 (Δ[HNO3])/(Δt) = -(Δ[Al2(CO3)3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[CO2])/(Δt) = 1/2 (Δ[Al(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Al2(CO3)3 ⟶ H_2O + CO_2 + Al(NO_3)_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: 6 HNO_3 + Al2(CO3)3 ⟶ 3 H_2O + 3 CO_2 + 2 Al(NO_3)_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 HNO_3 | 6 | -6 Al2(CO3)3 | 1 | -1 H_2O | 3 | 3 CO_2 | 3 | 3 Al(NO_3)_3 | 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 HNO_3 | 6 | -6 | -1/6 (Δ[HNO3])/(Δt) Al2(CO3)3 | 1 | -1 | -(Δ[Al2(CO3)3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) CO_2 | 3 | 3 | 1/3 (Δ[CO2])/(Δt) Al(NO_3)_3 | 2 | 2 | 1/2 (Δ[Al(NO3)3])/(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 = -1/6 (Δ[HNO3])/(Δt) = -(Δ[Al2(CO3)3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[CO2])/(Δt) = 1/2 (Δ[Al(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | Al2(CO3)3 | water | carbon dioxide | aluminum nitrate formula | HNO_3 | Al2(CO3)3 | H_2O | CO_2 | Al(NO_3)_3 Hill formula | HNO_3 | C3Al2O9 | H_2O | CO_2 | AlN_3O_9 name | nitric acid | | water | carbon dioxide | aluminum nitrate IUPAC name | nitric acid | | water | carbon dioxide | aluminum(+3) cation trinitrate
| nitric acid | Al2(CO3)3 | water | carbon dioxide | aluminum nitrate formula | HNO_3 | Al2(CO3)3 | H_2O | CO_2 | Al(NO_3)_3 Hill formula | HNO_3 | C3Al2O9 | H_2O | CO_2 | AlN_3O_9 name | nitric acid | | water | carbon dioxide | aluminum nitrate IUPAC name | nitric acid | | water | carbon dioxide | aluminum(+3) cation trinitrate

Substance properties

| nitric acid | Al2(CO3)3 | water | carbon dioxide | aluminum nitrate molar mass | 63.012 g/mol | 233.99 g/mol | 18.015 g/mol | 44.009 g/mol | 212.99 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | | 0 °C | -56.56 °C (at triple point) | 72.8 °C boiling point | 83 °C | | 99.9839 °C | -78.5 °C (at sublimation point) | density | 1.5129 g/cm^3 | | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 1.401 g/cm^3 solubility in water | miscible | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | 0.001338 Pa s (at 22 °C) odor | | | odorless | odorless |
| nitric acid | Al2(CO3)3 | water | carbon dioxide | aluminum nitrate molar mass | 63.012 g/mol | 233.99 g/mol | 18.015 g/mol | 44.009 g/mol | 212.99 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | | 0 °C | -56.56 °C (at triple point) | 72.8 °C boiling point | 83 °C | | 99.9839 °C | -78.5 °C (at sublimation point) | density | 1.5129 g/cm^3 | | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 1.401 g/cm^3 solubility in water | miscible | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | 0.001338 Pa s (at 22 °C) odor | | | odorless | odorless |

Units

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