Input interpretation
![Ca(OH)_2 (calcium hydroxide) + H_2CO_3 (carbonic acid) ⟶ H_2O (water) + CaCO_3 (calcium carbonate)](../image_source/6cfefdfe0b09f817fd10c9f0d7b4bff1.png)
Ca(OH)_2 (calcium hydroxide) + H_2CO_3 (carbonic acid) ⟶ H_2O (water) + CaCO_3 (calcium carbonate)
Balanced equation
![Balance the chemical equation algebraically: Ca(OH)_2 + H_2CO_3 ⟶ H_2O + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 H_2CO_3 ⟶ c_3 H_2O + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O and C: Ca: | c_1 = c_4 H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 2 c_1 + 3 c_2 = c_3 + 3 c_4 C: | 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_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: | | Ca(OH)_2 + H_2CO_3 ⟶ 2 H_2O + CaCO_3](../image_source/d2b269b5355c1bbb445fad82773b32c6.png)
Balance the chemical equation algebraically: Ca(OH)_2 + H_2CO_3 ⟶ H_2O + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 H_2CO_3 ⟶ c_3 H_2O + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O and C: Ca: | c_1 = c_4 H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 2 c_1 + 3 c_2 = c_3 + 3 c_4 C: | 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_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: | | Ca(OH)_2 + H_2CO_3 ⟶ 2 H_2O + CaCO_3
Structures
![+ ⟶ +](../image_source/c447188bee8d7b92b70efaee1c377da7.png)
+ ⟶ +
Names
![calcium hydroxide + carbonic acid ⟶ water + calcium carbonate](../image_source/fbc202111174d817313e30f406c1e4de.png)
calcium hydroxide + carbonic acid ⟶ water + calcium carbonate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Ca(OH)_2 + H_2CO_3 ⟶ H_2O + 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(OH)_2 + H_2CO_3 ⟶ 2 H_2O + 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(OH)_2 | 1 | -1 H_2CO_3 | 1 | -1 H_2O | 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 Ca(OH)_2 | 1 | -1 | ([Ca(OH)2])^(-1) H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) H_2O | 2 | 2 | ([H2O])^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 = ([Ca(OH)2])^(-1) ([H2CO3])^(-1) ([H2O])^2 [CaCO3] = (([H2O])^2 [CaCO3])/([Ca(OH)2] [H2CO3])](../image_source/f6c556e01b5183a41969fdf7d79b3e4f.png)
Construct the equilibrium constant, K, expression for: Ca(OH)_2 + H_2CO_3 ⟶ H_2O + 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(OH)_2 + H_2CO_3 ⟶ 2 H_2O + 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(OH)_2 | 1 | -1 H_2CO_3 | 1 | -1 H_2O | 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 Ca(OH)_2 | 1 | -1 | ([Ca(OH)2])^(-1) H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) H_2O | 2 | 2 | ([H2O])^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 = ([Ca(OH)2])^(-1) ([H2CO3])^(-1) ([H2O])^2 [CaCO3] = (([H2O])^2 [CaCO3])/([Ca(OH)2] [H2CO3])
Rate of reaction
![Construct the rate of reaction expression for: Ca(OH)_2 + H_2CO_3 ⟶ H_2O + 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(OH)_2 + H_2CO_3 ⟶ 2 H_2O + 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(OH)_2 | 1 | -1 H_2CO_3 | 1 | -1 H_2O | 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 Ca(OH)_2 | 1 | -1 | -(Δ[Ca(OH)2])/(Δt) H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(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(OH)2])/(Δt) = -(Δ[H2CO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/9b77c6952949f79f629925fcdf55abfe.png)
Construct the rate of reaction expression for: Ca(OH)_2 + H_2CO_3 ⟶ H_2O + 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(OH)_2 + H_2CO_3 ⟶ 2 H_2O + 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(OH)_2 | 1 | -1 H_2CO_3 | 1 | -1 H_2O | 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 Ca(OH)_2 | 1 | -1 | -(Δ[Ca(OH)2])/(Δt) H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(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(OH)2])/(Δt) = -(Δ[H2CO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| calcium hydroxide | carbonic acid | water | calcium carbonate formula | Ca(OH)_2 | H_2CO_3 | H_2O | CaCO_3 Hill formula | CaH_2O_2 | CH_2O_3 | H_2O | CCaO_3 name | calcium hydroxide | carbonic acid | water | calcium carbonate IUPAC name | calcium dihydroxide | carbonic acid | water | calcium carbonate](../image_source/4fe537780970708808b42ea8cfc9a2af.png)
| calcium hydroxide | carbonic acid | water | calcium carbonate formula | Ca(OH)_2 | H_2CO_3 | H_2O | CaCO_3 Hill formula | CaH_2O_2 | CH_2O_3 | H_2O | CCaO_3 name | calcium hydroxide | carbonic acid | water | calcium carbonate IUPAC name | calcium dihydroxide | carbonic acid | water | calcium carbonate
Substance properties
![| calcium hydroxide | carbonic acid | water | calcium carbonate molar mass | 74.092 g/mol | 62.024 g/mol | 18.015 g/mol | 100.09 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | 550 °C | | 0 °C | 1340 °C boiling point | | | 99.9839 °C | density | 2.24 g/cm^3 | | 1 g/cm^3 | 2.71 g/cm^3 solubility in water | slightly soluble | | | insoluble surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |](../image_source/bac0cdd04d3835f656b06fb6b9c506d0.png)
| calcium hydroxide | carbonic acid | water | calcium carbonate molar mass | 74.092 g/mol | 62.024 g/mol | 18.015 g/mol | 100.09 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) melting point | 550 °C | | 0 °C | 1340 °C boiling point | | | 99.9839 °C | density | 2.24 g/cm^3 | | 1 g/cm^3 | 2.71 g/cm^3 solubility in water | slightly soluble | | | insoluble surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |
Units