CaC2O4 = CO + CaCO3

CaC_2O_4 calcium oxalate ⟶ CO carbon monoxide + CaCO_3 calcium carbonate

Balance the chemical equation algebraically: CaC_2O_4 ⟶ CO + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaC_2O_4 ⟶ c_2 CO + c_3 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: | 2 c_1 = c_2 + c_3 Ca: | c_1 = c_3 O: | 4 c_1 = c_2 + 3 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CaC_2O_4 ⟶ CO + CaCO_3

⟶ +

calcium oxalate ⟶ carbon monoxide + calcium carbonate

Construct the equilibrium constant, K, expression for: CaC_2O_4 ⟶ CO + 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: CaC_2O_4 ⟶ CO + 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 CaC_2O_4 | 1 | -1 CO | 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 CaC_2O_4 | 1 | -1 | ([CaC2O4])^(-1) CO | 1 | 1 | [CO] 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 = ([CaC2O4])^(-1) [CO] [CaCO3] = ([CO] [CaCO3])/([CaC2O4])

Construct the rate of reaction expression for: CaC_2O_4 ⟶ CO + 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: CaC_2O_4 ⟶ CO + 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 CaC_2O_4 | 1 | -1 CO | 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 CaC_2O_4 | 1 | -1 | -(Δ[CaC2O4])/(Δt) CO | 1 | 1 | (Δ[CO])/(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[CaC2O4])/(Δt) = (Δ[CO])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| calcium oxalate | carbon monoxide | calcium carbonate formula | CaC_2O_4 | CO | CaCO_3 Hill formula | C_2CaO_4 | CO | CCaO_3 name | calcium oxalate | carbon monoxide | calcium carbonate

| calcium oxalate | carbon monoxide | calcium carbonate molar mass | 128.1 g/mol | 28.01 g/mol | 100.09 g/mol phase | | gas (at STP) | solid (at STP) melting point | | -205 °C | 1340 °C boiling point | | -191.5 °C | density | 2.2 g/cm^3 | 0.001145 g/cm^3 (at 25 °C) | 2.71 g/cm^3 solubility in water | | | insoluble dynamic viscosity | | 1.772×10^-5 Pa s (at 25 °C) | odor | | odorless |