Search

H2CO3 + Ca(NO3)2 = HNO3 + CaCO3

Input interpretation

H_2CO_3 carbonic acid + Ca(NO_3)_2 calcium nitrate ⟶ HNO_3 nitric acid + CaCO_3 calcium carbonate
H_2CO_3 carbonic acid + Ca(NO_3)_2 calcium nitrate ⟶ HNO_3 nitric acid + CaCO_3 calcium carbonate

Balanced equation

Balance the chemical equation algebraically: H_2CO_3 + Ca(NO_3)_2 ⟶ HNO_3 + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2CO_3 + c_2 Ca(NO_3)_2 ⟶ c_3 HNO_3 + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, H, O, Ca and N: C: | c_1 = c_4 H: | 2 c_1 = c_3 O: | 3 c_1 + 6 c_2 = 3 c_3 + 3 c_4 Ca: | c_2 = c_4 N: | 2 c_2 = c_3 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2CO_3 + Ca(NO_3)_2 ⟶ 2 HNO_3 + CaCO_3
Balance the chemical equation algebraically: H_2CO_3 + Ca(NO_3)_2 ⟶ HNO_3 + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2CO_3 + c_2 Ca(NO_3)_2 ⟶ c_3 HNO_3 + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, H, O, Ca and N: C: | c_1 = c_4 H: | 2 c_1 = c_3 O: | 3 c_1 + 6 c_2 = 3 c_3 + 3 c_4 Ca: | c_2 = c_4 N: | 2 c_2 = c_3 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2CO_3 + Ca(NO_3)_2 ⟶ 2 HNO_3 + CaCO_3

Structures

+ ⟶ +
+ ⟶ +

Names

carbonic acid + calcium nitrate ⟶ nitric acid + calcium carbonate
carbonic acid + calcium nitrate ⟶ nitric acid + calcium carbonate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2CO_3 + Ca(NO_3)_2 ⟶ HNO_3 + CaCO_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: H_2CO_3 + Ca(NO_3)_2 ⟶ 2 HNO_3 + CaCO_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 H_2CO_3 | 1 | -1 Ca(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 CaCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) Ca(NO_3)_2 | 1 | -1 | ([Ca(NO3)2])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 CaCO_3 | 1 | 1 | [CaCO3] 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 = ([H2CO3])^(-1) ([Ca(NO3)2])^(-1) ([HNO3])^2 [CaCO3] = (([HNO3])^2 [CaCO3])/([H2CO3] [Ca(NO3)2])
Construct the equilibrium constant, K, expression for: H_2CO_3 + Ca(NO_3)_2 ⟶ HNO_3 + CaCO_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: H_2CO_3 + Ca(NO_3)_2 ⟶ 2 HNO_3 + CaCO_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 H_2CO_3 | 1 | -1 Ca(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 CaCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) Ca(NO_3)_2 | 1 | -1 | ([Ca(NO3)2])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 CaCO_3 | 1 | 1 | [CaCO3] 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 = ([H2CO3])^(-1) ([Ca(NO3)2])^(-1) ([HNO3])^2 [CaCO3] = (([HNO3])^2 [CaCO3])/([H2CO3] [Ca(NO3)2])

Rate of reaction

Construct the rate of reaction expression for: H_2CO_3 + Ca(NO_3)_2 ⟶ HNO_3 + CaCO_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: H_2CO_3 + Ca(NO_3)_2 ⟶ 2 HNO_3 + CaCO_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 H_2CO_3 | 1 | -1 Ca(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 CaCO_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 H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) Ca(NO_3)_2 | 1 | -1 | -(Δ[Ca(NO3)2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) CaCO_3 | 1 | 1 | (Δ[CaCO3])/(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[H2CO3])/(Δt) = -(Δ[Ca(NO3)2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2CO_3 + Ca(NO_3)_2 ⟶ HNO_3 + CaCO_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: H_2CO_3 + Ca(NO_3)_2 ⟶ 2 HNO_3 + CaCO_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 H_2CO_3 | 1 | -1 Ca(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 CaCO_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 H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) Ca(NO_3)_2 | 1 | -1 | -(Δ[Ca(NO3)2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) CaCO_3 | 1 | 1 | (Δ[CaCO3])/(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[H2CO3])/(Δt) = -(Δ[Ca(NO3)2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| carbonic acid | calcium nitrate | nitric acid | calcium carbonate formula | H_2CO_3 | Ca(NO_3)_2 | HNO_3 | CaCO_3 Hill formula | CH_2O_3 | CaN_2O_6 | HNO_3 | CCaO_3 name | carbonic acid | calcium nitrate | nitric acid | calcium carbonate IUPAC name | carbonic acid | calcium dinitrate | nitric acid | calcium carbonate
| carbonic acid | calcium nitrate | nitric acid | calcium carbonate formula | H_2CO_3 | Ca(NO_3)_2 | HNO_3 | CaCO_3 Hill formula | CH_2O_3 | CaN_2O_6 | HNO_3 | CCaO_3 name | carbonic acid | calcium nitrate | nitric acid | calcium carbonate IUPAC name | carbonic acid | calcium dinitrate | nitric acid | calcium carbonate

Substance properties

| carbonic acid | calcium nitrate | nitric acid | calcium carbonate molar mass | 62.024 g/mol | 164.09 g/mol | 63.012 g/mol | 100.09 g/mol phase | | solid (at STP) | liquid (at STP) | solid (at STP) melting point | | 562 °C | -41.6 °C | 1340 °C boiling point | | | 83 °C | density | | 2.5 g/cm^3 | 1.5129 g/cm^3 | 2.71 g/cm^3 solubility in water | | soluble | miscible | insoluble dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) |
| carbonic acid | calcium nitrate | nitric acid | calcium carbonate molar mass | 62.024 g/mol | 164.09 g/mol | 63.012 g/mol | 100.09 g/mol phase | | solid (at STP) | liquid (at STP) | solid (at STP) melting point | | 562 °C | -41.6 °C | 1340 °C boiling point | | | 83 °C | density | | 2.5 g/cm^3 | 1.5129 g/cm^3 | 2.71 g/cm^3 solubility in water | | soluble | miscible | insoluble dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) |

Units

Random Queries

group of selenium vs tellurium
ion class of oxygen(I) cation vs cobalt(III) cation
formula of polybarit
formula of 4-nitro-2-(trifluoromethyl)benzonitrile
chemical types of dysprosium hydride vs gadolinium(III) nitrate hexahydrate
freezing point of 1,1,2-trichlorotrifluoroethane vs ethyl fluoride
alternate names of rhenium ditelluride
formula of rubidium cation vs sodium cation
alternate names of selenium(IV) ions
molar mass of group 12 ions