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HCl + Ca3N2 = CaCl2 + NH4Cl

Input interpretation

HCl hydrogen chloride + Ca_3N_2 calcium nitride ⟶ CaCl_2 calcium chloride + NH_4Cl ammonium chloride
HCl hydrogen chloride + Ca_3N_2 calcium nitride ⟶ CaCl_2 calcium chloride + NH_4Cl ammonium chloride

Balanced equation

Balance the chemical equation algebraically: HCl + Ca_3N_2 ⟶ CaCl_2 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Ca_3N_2 ⟶ c_3 CaCl_2 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Ca and N: Cl: | c_1 = 2 c_3 + c_4 H: | c_1 = 4 c_4 Ca: | 3 c_2 = c_3 N: | 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HCl + Ca_3N_2 ⟶ 3 CaCl_2 + 2 NH_4Cl
Balance the chemical equation algebraically: HCl + Ca_3N_2 ⟶ CaCl_2 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Ca_3N_2 ⟶ c_3 CaCl_2 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Ca and N: Cl: | c_1 = 2 c_3 + c_4 H: | c_1 = 4 c_4 Ca: | 3 c_2 = c_3 N: | 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 1 c_3 = 3 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 HCl + Ca_3N_2 ⟶ 3 CaCl_2 + 2 NH_4Cl

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen chloride + calcium nitride ⟶ calcium chloride + ammonium chloride
hydrogen chloride + calcium nitride ⟶ calcium chloride + ammonium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + Ca_3N_2 ⟶ CaCl_2 + 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: 8 HCl + Ca_3N_2 ⟶ 3 CaCl_2 + 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 HCl | 8 | -8 Ca_3N_2 | 1 | -1 CaCl_2 | 3 | 3 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 HCl | 8 | -8 | ([HCl])^(-8) Ca_3N_2 | 1 | -1 | ([Ca3N2])^(-1) CaCl_2 | 3 | 3 | ([CaCl2])^3 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 = ([HCl])^(-8) ([Ca3N2])^(-1) ([CaCl2])^3 ([NH4Cl])^2 = (([CaCl2])^3 ([NH4Cl])^2)/(([HCl])^8 [Ca3N2])
Construct the equilibrium constant, K, expression for: HCl + Ca_3N_2 ⟶ CaCl_2 + 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: 8 HCl + Ca_3N_2 ⟶ 3 CaCl_2 + 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 HCl | 8 | -8 Ca_3N_2 | 1 | -1 CaCl_2 | 3 | 3 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 HCl | 8 | -8 | ([HCl])^(-8) Ca_3N_2 | 1 | -1 | ([Ca3N2])^(-1) CaCl_2 | 3 | 3 | ([CaCl2])^3 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 = ([HCl])^(-8) ([Ca3N2])^(-1) ([CaCl2])^3 ([NH4Cl])^2 = (([CaCl2])^3 ([NH4Cl])^2)/(([HCl])^8 [Ca3N2])

Rate of reaction

Construct the rate of reaction expression for: HCl + Ca_3N_2 ⟶ CaCl_2 + 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: 8 HCl + Ca_3N_2 ⟶ 3 CaCl_2 + 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 HCl | 8 | -8 Ca_3N_2 | 1 | -1 CaCl_2 | 3 | 3 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 HCl | 8 | -8 | -1/8 (Δ[HCl])/(Δt) Ca_3N_2 | 1 | -1 | -(Δ[Ca3N2])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(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 = -1/8 (Δ[HCl])/(Δt) = -(Δ[Ca3N2])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + Ca_3N_2 ⟶ CaCl_2 + 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: 8 HCl + Ca_3N_2 ⟶ 3 CaCl_2 + 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 HCl | 8 | -8 Ca_3N_2 | 1 | -1 CaCl_2 | 3 | 3 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 HCl | 8 | -8 | -1/8 (Δ[HCl])/(Δt) Ca_3N_2 | 1 | -1 | -(Δ[Ca3N2])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(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 = -1/8 (Δ[HCl])/(Δt) = -(Δ[Ca3N2])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | calcium nitride | calcium chloride | ammonium chloride formula | HCl | Ca_3N_2 | CaCl_2 | NH_4Cl Hill formula | ClH | Ca_3N_2 | CaCl_2 | ClH_4N name | hydrogen chloride | calcium nitride | calcium chloride | ammonium chloride IUPAC name | hydrogen chloride | calcium azanidylidenecalcium | calcium dichloride | ammonium chloride
| hydrogen chloride | calcium nitride | calcium chloride | ammonium chloride formula | HCl | Ca_3N_2 | CaCl_2 | NH_4Cl Hill formula | ClH | Ca_3N_2 | CaCl_2 | ClH_4N name | hydrogen chloride | calcium nitride | calcium chloride | ammonium chloride IUPAC name | hydrogen chloride | calcium azanidylidenecalcium | calcium dichloride | ammonium chloride

Substance properties

| hydrogen chloride | calcium nitride | calcium chloride | ammonium chloride molar mass | 36.46 g/mol | 148.25 g/mol | 111 g/mol | 53.49 g/mol phase | gas (at STP) | | solid (at STP) | solid (at STP) melting point | -114.17 °C | | 772 °C | 340 °C boiling point | -85 °C | | | density | 0.00149 g/cm^3 (at 25 °C) | 2.63 g/cm^3 | 2.15 g/cm^3 | 1.5256 g/cm^3 solubility in water | miscible | | soluble | soluble
| hydrogen chloride | calcium nitride | calcium chloride | ammonium chloride molar mass | 36.46 g/mol | 148.25 g/mol | 111 g/mol | 53.49 g/mol phase | gas (at STP) | | solid (at STP) | solid (at STP) melting point | -114.17 °C | | 772 °C | 340 °C boiling point | -85 °C | | | density | 0.00149 g/cm^3 (at 25 °C) | 2.63 g/cm^3 | 2.15 g/cm^3 | 1.5256 g/cm^3 solubility in water | miscible | | soluble | soluble

Units

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