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NaNO3 + NH4Cl = NaCl + NH4NO3

Input interpretation

NaNO_3 sodium nitrate + NH_4Cl ammonium chloride ⟶ NaCl sodium chloride + NH_4NO_3 ammonium nitrate
NaNO_3 sodium nitrate + NH_4Cl ammonium chloride ⟶ NaCl sodium chloride + NH_4NO_3 ammonium nitrate

Balanced equation

Balance the chemical equation algebraically: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaNO_3 + c_2 NH_4Cl ⟶ c_3 NaCl + c_4 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for N, Na, O, Cl and H: N: | c_1 + c_2 = 2 c_4 Na: | c_1 = c_3 O: | 3 c_1 = 3 c_4 Cl: | c_2 = c_3 H: | 4 c_2 = 4 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_3
Balance the chemical equation algebraically: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaNO_3 + c_2 NH_4Cl ⟶ c_3 NaCl + c_4 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for N, Na, O, Cl and H: N: | c_1 + c_2 = 2 c_4 Na: | c_1 = c_3 O: | 3 c_1 = 3 c_4 Cl: | c_2 = c_3 H: | 4 c_2 = 4 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_3

Structures

+ ⟶ +
+ ⟶ +

Names

sodium nitrate + ammonium chloride ⟶ sodium chloride + ammonium nitrate
sodium nitrate + ammonium chloride ⟶ sodium chloride + ammonium nitrate

Reaction thermodynamics

Gibbs free energy

| sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate molecular free energy | -366 kJ/mol | -202.9 kJ/mol | -384.1 kJ/mol | -183.9 kJ/mol total free energy | -366 kJ/mol | -202.9 kJ/mol | -384.1 kJ/mol | -183.9 kJ/mol | G_initial = -568.9 kJ/mol | | G_final = -568 kJ/mol | ΔG_rxn^0 | -568 kJ/mol - -568.9 kJ/mol = 0.9 kJ/mol (endergonic) | | |
| sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate molecular free energy | -366 kJ/mol | -202.9 kJ/mol | -384.1 kJ/mol | -183.9 kJ/mol total free energy | -366 kJ/mol | -202.9 kJ/mol | -384.1 kJ/mol | -183.9 kJ/mol | G_initial = -568.9 kJ/mol | | G_final = -568 kJ/mol | ΔG_rxn^0 | -568 kJ/mol - -568.9 kJ/mol = 0.9 kJ/mol (endergonic) | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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 NaNO_3 | 1 | -1 NH_4Cl | 1 | -1 NaCl | 1 | 1 NH_4NO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaNO_3 | 1 | -1 | ([NaNO3])^(-1) NH_4Cl | 1 | -1 | ([NH4Cl])^(-1) NaCl | 1 | 1 | [NaCl] NH_4NO_3 | 1 | 1 | [NH4NO3] 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 = ([NaNO3])^(-1) ([NH4Cl])^(-1) [NaCl] [NH4NO3] = ([NaCl] [NH4NO3])/([NaNO3] [NH4Cl])
Construct the equilibrium constant, K, expression for: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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 NaNO_3 | 1 | -1 NH_4Cl | 1 | -1 NaCl | 1 | 1 NH_4NO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaNO_3 | 1 | -1 | ([NaNO3])^(-1) NH_4Cl | 1 | -1 | ([NH4Cl])^(-1) NaCl | 1 | 1 | [NaCl] NH_4NO_3 | 1 | 1 | [NH4NO3] 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 = ([NaNO3])^(-1) ([NH4Cl])^(-1) [NaCl] [NH4NO3] = ([NaCl] [NH4NO3])/([NaNO3] [NH4Cl])

Rate of reaction

Construct the rate of reaction expression for: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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 NaNO_3 | 1 | -1 NH_4Cl | 1 | -1 NaCl | 1 | 1 NH_4NO_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 NaNO_3 | 1 | -1 | -(Δ[NaNO3])/(Δt) NH_4Cl | 1 | -1 | -(Δ[NH4Cl])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) NH_4NO_3 | 1 | 1 | (Δ[NH4NO3])/(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[NaNO3])/(Δt) = -(Δ[NH4Cl])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[NH4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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: NaNO_3 + NH_4Cl ⟶ NaCl + NH_4NO_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 NaNO_3 | 1 | -1 NH_4Cl | 1 | -1 NaCl | 1 | 1 NH_4NO_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 NaNO_3 | 1 | -1 | -(Δ[NaNO3])/(Δt) NH_4Cl | 1 | -1 | -(Δ[NH4Cl])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) NH_4NO_3 | 1 | 1 | (Δ[NH4NO3])/(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[NaNO3])/(Δt) = -(Δ[NH4Cl])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[NH4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate formula | NaNO_3 | NH_4Cl | NaCl | NH_4NO_3 Hill formula | NNaO_3 | ClH_4N | ClNa | H_4N_2O_3 name | sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate
| sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate formula | NaNO_3 | NH_4Cl | NaCl | NH_4NO_3 Hill formula | NNaO_3 | ClH_4N | ClNa | H_4N_2O_3 name | sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate

Substance properties

| sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate molar mass | 84.994 g/mol | 53.49 g/mol | 58.44 g/mol | 80.04 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 306 °C | 340 °C | 801 °C | 169 °C boiling point | | | 1413 °C | 210 °C density | 2.26 g/cm^3 | 1.5256 g/cm^3 | 2.16 g/cm^3 | 1.73 g/cm^3 solubility in water | soluble | soluble | soluble | dynamic viscosity | 0.003 Pa s (at 250 °C) | | | odor | | | odorless | odorless
| sodium nitrate | ammonium chloride | sodium chloride | ammonium nitrate molar mass | 84.994 g/mol | 53.49 g/mol | 58.44 g/mol | 80.04 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 306 °C | 340 °C | 801 °C | 169 °C boiling point | | | 1413 °C | 210 °C density | 2.26 g/cm^3 | 1.5256 g/cm^3 | 2.16 g/cm^3 | 1.73 g/cm^3 solubility in water | soluble | soluble | soluble | dynamic viscosity | 0.003 Pa s (at 250 °C) | | | odor | | | odorless | odorless

Units

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