Input interpretation
![Ca(HCO3)2 ⟶ H_2O (water) + CO_2 (carbon dioxide) + CaCO_3 (calcium carbonate)](../image_source/f68be8457e2b50f47a03452f43ac75b3.png)
Ca(HCO3)2 ⟶ H_2O (water) + CO_2 (carbon dioxide) + CaCO_3 (calcium carbonate)
Balanced equation
![Balance the chemical equation algebraically: Ca(HCO3)2 ⟶ H_2O + CO_2 + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(HCO3)2 ⟶ c_2 H_2O + c_3 CO_2 + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, C and O: Ca: | c_1 = c_4 H: | 2 c_1 = 2 c_2 C: | 2 c_1 = c_3 + c_4 O: | 6 c_1 = c_2 + 2 c_3 + 3 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: | | Ca(HCO3)2 ⟶ H_2O + CO_2 + CaCO_3](../image_source/895983ead5b065c59bba9fab359ef1bc.png)
Balance the chemical equation algebraically: Ca(HCO3)2 ⟶ H_2O + CO_2 + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(HCO3)2 ⟶ c_2 H_2O + c_3 CO_2 + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, C and O: Ca: | c_1 = c_4 H: | 2 c_1 = 2 c_2 C: | 2 c_1 = c_3 + c_4 O: | 6 c_1 = c_2 + 2 c_3 + 3 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: | | Ca(HCO3)2 ⟶ H_2O + CO_2 + CaCO_3
Structures
![Ca(HCO3)2 ⟶ + +](../image_source/13439862267827c0ad0b5664baa6e966.png)
Ca(HCO3)2 ⟶ + +
Names
![Ca(HCO3)2 ⟶ water + carbon dioxide + calcium carbonate](../image_source/1e5b569fcdbf26b8f576037d86a16a5a.png)
Ca(HCO3)2 ⟶ water + carbon dioxide + calcium carbonate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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 Ca(HCO3)2 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 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 Ca(HCO3)2 | 1 | -1 | ([Ca(HCO3)2])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] 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 = ([Ca(HCO3)2])^(-1) [H2O] [CO2] [CaCO3] = ([H2O] [CO2] [CaCO3])/([Ca(HCO3)2])](../image_source/359ae8e327aa408c897aafc965a798fa.png)
Construct the equilibrium constant, K, expression for: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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 Ca(HCO3)2 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 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 Ca(HCO3)2 | 1 | -1 | ([Ca(HCO3)2])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] 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 = ([Ca(HCO3)2])^(-1) [H2O] [CO2] [CaCO3] = ([H2O] [CO2] [CaCO3])/([Ca(HCO3)2])
Rate of reaction
![Construct the rate of reaction expression for: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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 Ca(HCO3)2 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 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 Ca(HCO3)2 | 1 | -1 | -(Δ[Ca(HCO3)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(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[Ca(HCO3)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/24d38e62fd33601acf99a9d624cce009.png)
Construct the rate of reaction expression for: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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: Ca(HCO3)2 ⟶ H_2O + CO_2 + 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 Ca(HCO3)2 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 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 Ca(HCO3)2 | 1 | -1 | -(Δ[Ca(HCO3)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(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[Ca(HCO3)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| Ca(HCO3)2 | water | carbon dioxide | calcium carbonate formula | Ca(HCO3)2 | H_2O | CO_2 | CaCO_3 Hill formula | C2H2CaO6 | H_2O | CO_2 | CCaO_3 name | | water | carbon dioxide | calcium carbonate](../image_source/8104f358846f76dd6351195b7392961f.png)
| Ca(HCO3)2 | water | carbon dioxide | calcium carbonate formula | Ca(HCO3)2 | H_2O | CO_2 | CaCO_3 Hill formula | C2H2CaO6 | H_2O | CO_2 | CCaO_3 name | | water | carbon dioxide | calcium carbonate
Substance properties
![| Ca(HCO3)2 | water | carbon dioxide | calcium carbonate molar mass | 162.11 g/mol | 18.015 g/mol | 44.009 g/mol | 100.09 g/mol phase | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | | 0 °C | -56.56 °C (at triple point) | 1340 °C boiling point | | 99.9839 °C | -78.5 °C (at sublimation point) | density | | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 2.71 g/cm^3 solubility in water | | | | insoluble surface tension | | 0.0728 N/m | | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless |](../image_source/70128c6f9cffee2a53d1d64d18c0f73e.png)
| Ca(HCO3)2 | water | carbon dioxide | calcium carbonate molar mass | 162.11 g/mol | 18.015 g/mol | 44.009 g/mol | 100.09 g/mol phase | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | | 0 °C | -56.56 °C (at triple point) | 1340 °C boiling point | | 99.9839 °C | -78.5 °C (at sublimation point) | density | | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | 2.71 g/cm^3 solubility in water | | | | insoluble surface tension | | 0.0728 N/m | | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | odor | | odorless | odorless |
Units