CaOCO2 = CaCO3

CaCO_3 calcium carbonate ⟶ CaCO_3 calcium carbonate

Balance the chemical equation algebraically: CaCO_3 ⟶ CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCO_3 ⟶ c_2 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, Ca and O: C: | c_1 = c_2 Ca: | c_1 = c_2 O: | 3 c_1 = 3 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: | | CaCO_3 ⟶ CaCO_3

⟶

calcium carbonate ⟶ calcium carbonate

| calcium carbonate | calcium carbonate molecular enthalpy | -1208 kJ/mol | -1208 kJ/mol total enthalpy | -1208 kJ/mol | -1208 kJ/mol | H_initial = -1208 kJ/mol | H_final = -1208 kJ/mol ΔH_rxn^0 | -1208 kJ/mol - -1208 kJ/mol = 0 kJ/mol (equilibrium) |

| calcium carbonate | calcium carbonate molecular free energy | -1129 kJ/mol | -1129 kJ/mol total free energy | -1129 kJ/mol | -1129 kJ/mol | G_initial = -1129 kJ/mol | G_final = -1129 kJ/mol ΔG_rxn^0 | -1129 kJ/mol - -1129 kJ/mol = 0 kJ/mol (equilibrium) |

| calcium carbonate | calcium carbonate molecular entropy | 91.7 J/(mol K) | 91.7 J/(mol K) total entropy | 91.7 J/(mol K) | 91.7 J/(mol K) | S_initial = 91.7 J/(mol K) | S_final = 91.7 J/(mol K) ΔS_rxn^0 | 91.7 J/(mol K) - 91.7 J/(mol K) = 0 J/(mol K) (equilibrium) |

Construct the equilibrium constant, K, expression for: CaCO_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: CaCO_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 CaCO_3 | 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 CaCO_3 | 1 | -1 | ([CaCO3])^(-1) 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 = ([CaCO3])^(-1) [CaCO3] = ([CaCO3])/([CaCO3])

Construct the rate of reaction expression for: CaCO_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: CaCO_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 CaCO_3 | 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 CaCO_3 | 1 | -1 | -(Δ[CaCO3])/(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[CaCO3])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| calcium carbonate | calcium carbonate formula | CaCO_3 | CaCO_3 Hill formula | CCaO_3 | CCaO_3 name | calcium carbonate | calcium carbonate

| calcium carbonate | calcium carbonate molar mass | 100.09 g/mol | 100.09 g/mol phase | solid (at STP) | solid (at STP) melting point | 1340 °C | 1340 °C density | 2.71 g/cm^3 | 2.71 g/cm^3 solubility in water | insoluble | insoluble