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CaCl2 + (NH4)2CO3 = CaCO3 + NH4Cl

Input interpretation

CaCl_2 calcium chloride + (NH_4)_2CO_3 ammonium carbonate ⟶ CaCO_3 calcium carbonate + NH_4Cl ammonium chloride
CaCl_2 calcium chloride + (NH_4)_2CO_3 ammonium carbonate ⟶ CaCO_3 calcium carbonate + NH_4Cl ammonium chloride

Balanced equation

Balance the chemical equation algebraically: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCl_2 + c_2 (NH_4)_2CO_3 ⟶ c_3 CaCO_3 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl, C, H, N and O: Ca: | c_1 = c_3 Cl: | 2 c_1 = c_4 C: | c_2 = c_3 H: | 8 c_2 = 4 c_4 N: | 2 c_2 = c_4 O: | 3 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 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + 2 NH_4Cl
Balance the chemical equation algebraically: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCl_2 + c_2 (NH_4)_2CO_3 ⟶ c_3 CaCO_3 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl, C, H, N and O: Ca: | c_1 = c_3 Cl: | 2 c_1 = c_4 C: | c_2 = c_3 H: | 8 c_2 = 4 c_4 N: | 2 c_2 = c_4 O: | 3 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 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + 2 NH_4Cl

Structures

+ ⟶ +
+ ⟶ +

Names

calcium chloride + ammonium carbonate ⟶ calcium carbonate + ammonium chloride
calcium chloride + ammonium carbonate ⟶ calcium carbonate + ammonium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + NH_4Cl 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: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + 2 NH_4Cl 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 CaCl_2 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 CaCO_3 | 1 | 1 NH_4Cl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaCl_2 | 1 | -1 | ([CaCl2])^(-1) (NH_4)_2CO_3 | 1 | -1 | ([(NH4)2CO3])^(-1) CaCO_3 | 1 | 1 | [CaCO3] NH_4Cl | 2 | 2 | ([NH4Cl])^2 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 = ([CaCl2])^(-1) ([(NH4)2CO3])^(-1) [CaCO3] ([NH4Cl])^2 = ([CaCO3] ([NH4Cl])^2)/([CaCl2] [(NH4)2CO3])
Construct the equilibrium constant, K, expression for: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + NH_4Cl 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: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + 2 NH_4Cl 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 CaCl_2 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 CaCO_3 | 1 | 1 NH_4Cl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaCl_2 | 1 | -1 | ([CaCl2])^(-1) (NH_4)_2CO_3 | 1 | -1 | ([(NH4)2CO3])^(-1) CaCO_3 | 1 | 1 | [CaCO3] NH_4Cl | 2 | 2 | ([NH4Cl])^2 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 = ([CaCl2])^(-1) ([(NH4)2CO3])^(-1) [CaCO3] ([NH4Cl])^2 = ([CaCO3] ([NH4Cl])^2)/([CaCl2] [(NH4)2CO3])

Rate of reaction

Construct the rate of reaction expression for: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + NH_4Cl 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: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + 2 NH_4Cl 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 CaCl_2 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 CaCO_3 | 1 | 1 NH_4Cl | 2 | 2 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 CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) (NH_4)_2CO_3 | 1 | -1 | -(Δ[(NH4)2CO3])/(Δt) CaCO_3 | 1 | 1 | (Δ[CaCO3])/(Δt) NH_4Cl | 2 | 2 | 1/2 (Δ[NH4Cl])/(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[CaCl2])/(Δt) = -(Δ[(NH4)2CO3])/(Δt) = (Δ[CaCO3])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + NH_4Cl 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: CaCl_2 + (NH_4)_2CO_3 ⟶ CaCO_3 + 2 NH_4Cl 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 CaCl_2 | 1 | -1 (NH_4)_2CO_3 | 1 | -1 CaCO_3 | 1 | 1 NH_4Cl | 2 | 2 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 CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) (NH_4)_2CO_3 | 1 | -1 | -(Δ[(NH4)2CO3])/(Δt) CaCO_3 | 1 | 1 | (Δ[CaCO3])/(Δt) NH_4Cl | 2 | 2 | 1/2 (Δ[NH4Cl])/(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[CaCl2])/(Δt) = -(Δ[(NH4)2CO3])/(Δt) = (Δ[CaCO3])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| calcium chloride | ammonium carbonate | calcium carbonate | ammonium chloride formula | CaCl_2 | (NH_4)_2CO_3 | CaCO_3 | NH_4Cl Hill formula | CaCl_2 | CH_8N_2O_3 | CCaO_3 | ClH_4N name | calcium chloride | ammonium carbonate | calcium carbonate | ammonium chloride IUPAC name | calcium dichloride | | calcium carbonate | ammonium chloride
| calcium chloride | ammonium carbonate | calcium carbonate | ammonium chloride formula | CaCl_2 | (NH_4)_2CO_3 | CaCO_3 | NH_4Cl Hill formula | CaCl_2 | CH_8N_2O_3 | CCaO_3 | ClH_4N name | calcium chloride | ammonium carbonate | calcium carbonate | ammonium chloride IUPAC name | calcium dichloride | | calcium carbonate | ammonium chloride

Substance properties

| calcium chloride | ammonium carbonate | calcium carbonate | ammonium chloride molar mass | 111 g/mol | 96.09 g/mol | 100.09 g/mol | 53.49 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 772 °C | 58 °C | 1340 °C | 340 °C density | 2.15 g/cm^3 | 1.5 g/cm^3 | 2.71 g/cm^3 | 1.5256 g/cm^3 solubility in water | soluble | soluble | insoluble | soluble
| calcium chloride | ammonium carbonate | calcium carbonate | ammonium chloride molar mass | 111 g/mol | 96.09 g/mol | 100.09 g/mol | 53.49 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 772 °C | 58 °C | 1340 °C | 340 °C density | 2.15 g/cm^3 | 1.5 g/cm^3 | 2.71 g/cm^3 | 1.5256 g/cm^3 solubility in water | soluble | soluble | insoluble | soluble

Units

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