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HNO3 + CaCO3 = H2O + CO2 + Ca(NO3)2

Input interpretation

HNO_3 (nitric acid) + CaCO_3 (calcium carbonate) ⟶ H_2O (water) + CO_2 (carbon dioxide) + Ca(NO_3)_2 (calcium nitrate)
HNO_3 (nitric acid) + CaCO_3 (calcium carbonate) ⟶ H_2O (water) + CO_2 (carbon dioxide) + Ca(NO_3)_2 (calcium nitrate)

Balanced equation

Balance the chemical equation algebraically: HNO_3 + CaCO_3 ⟶ H_2O + CO_2 + Ca(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 CaCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 Ca(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, C and Ca: H: | c_1 = 2 c_3 N: | c_1 = 2 c_5 O: | 3 c_1 + 3 c_2 = c_3 + 2 c_4 + 6 c_5 C: | c_2 = c_4 Ca: | c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 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: |   | 2 HNO_3 + CaCO_3 ⟶ H_2O + CO_2 + Ca(NO_3)_2
Balance the chemical equation algebraically: HNO_3 + CaCO_3 ⟶ H_2O + CO_2 + Ca(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 CaCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 Ca(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, C and Ca: H: | c_1 = 2 c_3 N: | c_1 = 2 c_5 O: | 3 c_1 + 3 c_2 = c_3 + 2 c_4 + 6 c_5 C: | c_2 = c_4 Ca: | c_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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 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: | | 2 HNO_3 + CaCO_3 ⟶ H_2O + CO_2 + Ca(NO_3)_2

Structures

 + ⟶ + +
+ ⟶ + +

Names

nitric acid + calcium carbonate ⟶ water + carbon dioxide + calcium nitrate
nitric acid + calcium carbonate ⟶ water + carbon dioxide + calcium nitrate

Reaction thermodynamics

Gibbs free energy

ΔG_rxn^0 | -1374 kJ/mol - -1291 kJ/mol = -83.8 kJ/mol (exergonic)
ΔG_rxn^0 | -1374 kJ/mol - -1291 kJ/mol = -83.8 kJ/mol (exergonic)

Units

Equilibrium constant

K_c = ([H2O] [CO2] [Ca(NO3)2])/([HNO3]^2 [CaCO3])
K_c = ([H2O] [CO2] [Ca(NO3)2])/([HNO3]^2 [CaCO3])

Rate of reaction

rate = -1/2 (Δ[HNO3])/(Δt) = -(Δ[CaCO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[Ca(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
rate = -1/2 (Δ[HNO3])/(Δt) = -(Δ[CaCO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[Ca(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | nitric acid | calcium carbonate | water | carbon dioxide | calcium nitrate formula | HNO_3 | CaCO_3 | H_2O | CO_2 | Ca(NO_3)_2 Hill formula | HNO_3 | CCaO_3 | H_2O | CO_2 | CaN_2O_6 name | nitric acid | calcium carbonate | water | carbon dioxide | calcium nitrate IUPAC name | nitric acid | calcium carbonate | water | carbon dioxide | calcium dinitrate
| nitric acid | calcium carbonate | water | carbon dioxide | calcium nitrate formula | HNO_3 | CaCO_3 | H_2O | CO_2 | Ca(NO_3)_2 Hill formula | HNO_3 | CCaO_3 | H_2O | CO_2 | CaN_2O_6 name | nitric acid | calcium carbonate | water | carbon dioxide | calcium nitrate IUPAC name | nitric acid | calcium carbonate | water | carbon dioxide | calcium dinitrate