Input interpretation
Ca(HCO3)2 ⟶ CaCO3CO2H2O
Balanced equation
Balance the chemical equation algebraically: Ca(HCO3)2 ⟶ CaCO3CO2H2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(HCO3)2 ⟶ c_2 CaCO3CO2H2O 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_2 H: | 2 c_1 = 2 c_2 C: | 2 c_1 = 2 c_2 O: | 6 c_1 = 6 c_2 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Ca(HCO3)2 ⟶ CaCO3CO2H2O
Structures
Ca(HCO3)2 ⟶ CaCO3CO2H2O
Names
Ca(HCO3)2 ⟶ CaCO3CO2H2O
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Ca(HCO3)2 ⟶ CaCO3CO2H2O 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 ⟶ CaCO3CO2H2O 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 CaCO3CO2H2O | 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) CaCO3CO2H2O | 1 | 1 | [CaCO3CO2H2O] 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) [CaCO3CO2H2O] = ([CaCO3CO2H2O])/([Ca(HCO3)2])](../image_source/536c25a4f964ba9d6c77930213fe3033.png)
Construct the equilibrium constant, K, expression for: Ca(HCO3)2 ⟶ CaCO3CO2H2O 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 ⟶ CaCO3CO2H2O 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 CaCO3CO2H2O | 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) CaCO3CO2H2O | 1 | 1 | [CaCO3CO2H2O] 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) [CaCO3CO2H2O] = ([CaCO3CO2H2O])/([Ca(HCO3)2])
Rate of reaction
![Construct the rate of reaction expression for: Ca(HCO3)2 ⟶ CaCO3CO2H2O 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 ⟶ CaCO3CO2H2O 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 CaCO3CO2H2O | 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) CaCO3CO2H2O | 1 | 1 | (Δ[CaCO3CO2H2O])/(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[CaCO3CO2H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/4fa53fb6d05df6d17efb1ee880d2027d.png)
Construct the rate of reaction expression for: Ca(HCO3)2 ⟶ CaCO3CO2H2O 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 ⟶ CaCO3CO2H2O 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 CaCO3CO2H2O | 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) CaCO3CO2H2O | 1 | 1 | (Δ[CaCO3CO2H2O])/(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[CaCO3CO2H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| Ca(HCO3)2 | CaCO3CO2H2O formula | Ca(HCO3)2 | CaCO3CO2H2O Hill formula | C2H2CaO6 | C2H2CaO6
Substance properties
| Ca(HCO3)2 | CaCO3CO2H2O molar mass | 162.11 g/mol | 162.11 g/mol
Units
