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NH4Cl + Na[Al(OH)4] = H2O + NaCl + NH3 + Al(OH)3

Input interpretation

NH_4Cl ammonium chloride + NaAl(OH)4 ⟶ H_2O water + NaCl sodium chloride + NH_3 ammonia + Al(OH)_3 aluminum hydroxide
NH_4Cl ammonium chloride + NaAl(OH)4 ⟶ H_2O water + NaCl sodium chloride + NH_3 ammonia + Al(OH)_3 aluminum hydroxide

Balanced equation

Balance the chemical equation algebraically: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_4Cl + c_2 NaAl(OH)4 ⟶ c_3 H_2O + c_4 NaCl + c_5 NH_3 + c_6 Al(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, Na, Al and O: Cl: | c_1 = c_4 H: | 4 c_1 + 4 c_2 = 2 c_3 + 3 c_5 + 3 c_6 N: | c_1 = c_5 Na: | c_2 = c_4 Al: | c_2 = c_6 O: | 4 c_2 = c_3 + 3 c_6 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 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_3
Balance the chemical equation algebraically: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_4Cl + c_2 NaAl(OH)4 ⟶ c_3 H_2O + c_4 NaCl + c_5 NH_3 + c_6 Al(OH)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, Na, Al and O: Cl: | c_1 = c_4 H: | 4 c_1 + 4 c_2 = 2 c_3 + 3 c_5 + 3 c_6 N: | c_1 = c_5 Na: | c_2 = c_4 Al: | c_2 = c_6 O: | 4 c_2 = c_3 + 3 c_6 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 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_3

Structures

+ NaAl(OH)4 ⟶ + + +
+ NaAl(OH)4 ⟶ + + +

Names

ammonium chloride + NaAl(OH)4 ⟶ water + sodium chloride + ammonia + aluminum hydroxide
ammonium chloride + NaAl(OH)4 ⟶ water + sodium chloride + ammonia + aluminum hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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 NH_4Cl | 1 | -1 NaAl(OH)4 | 1 | -1 H_2O | 1 | 1 NaCl | 1 | 1 NH_3 | 1 | 1 Al(OH)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_4Cl | 1 | -1 | ([NH4Cl])^(-1) NaAl(OH)4 | 1 | -1 | ([NaAl(OH)4])^(-1) H_2O | 1 | 1 | [H2O] NaCl | 1 | 1 | [NaCl] NH_3 | 1 | 1 | [NH3] Al(OH)_3 | 1 | 1 | [Al(OH)3] 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 = ([NH4Cl])^(-1) ([NaAl(OH)4])^(-1) [H2O] [NaCl] [NH3] [Al(OH)3] = ([H2O] [NaCl] [NH3] [Al(OH)3])/([NH4Cl] [NaAl(OH)4])
Construct the equilibrium constant, K, expression for: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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 NH_4Cl | 1 | -1 NaAl(OH)4 | 1 | -1 H_2O | 1 | 1 NaCl | 1 | 1 NH_3 | 1 | 1 Al(OH)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_4Cl | 1 | -1 | ([NH4Cl])^(-1) NaAl(OH)4 | 1 | -1 | ([NaAl(OH)4])^(-1) H_2O | 1 | 1 | [H2O] NaCl | 1 | 1 | [NaCl] NH_3 | 1 | 1 | [NH3] Al(OH)_3 | 1 | 1 | [Al(OH)3] 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 = ([NH4Cl])^(-1) ([NaAl(OH)4])^(-1) [H2O] [NaCl] [NH3] [Al(OH)3] = ([H2O] [NaCl] [NH3] [Al(OH)3])/([NH4Cl] [NaAl(OH)4])

Rate of reaction

Construct the rate of reaction expression for: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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 NH_4Cl | 1 | -1 NaAl(OH)4 | 1 | -1 H_2O | 1 | 1 NaCl | 1 | 1 NH_3 | 1 | 1 Al(OH)_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 NH_4Cl | 1 | -1 | -(Δ[NH4Cl])/(Δt) NaAl(OH)4 | 1 | -1 | -(Δ[NaAl(OH)4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) NH_3 | 1 | 1 | (Δ[NH3])/(Δt) Al(OH)_3 | 1 | 1 | (Δ[Al(OH)3])/(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[NH4Cl])/(Δt) = -(Δ[NaAl(OH)4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[NH3])/(Δt) = (Δ[Al(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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: NH_4Cl + NaAl(OH)4 ⟶ H_2O + NaCl + NH_3 + Al(OH)_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 NH_4Cl | 1 | -1 NaAl(OH)4 | 1 | -1 H_2O | 1 | 1 NaCl | 1 | 1 NH_3 | 1 | 1 Al(OH)_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 NH_4Cl | 1 | -1 | -(Δ[NH4Cl])/(Δt) NaAl(OH)4 | 1 | -1 | -(Δ[NaAl(OH)4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) NH_3 | 1 | 1 | (Δ[NH3])/(Δt) Al(OH)_3 | 1 | 1 | (Δ[Al(OH)3])/(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[NH4Cl])/(Δt) = -(Δ[NaAl(OH)4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[NH3])/(Δt) = (Δ[Al(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| ammonium chloride | NaAl(OH)4 | water | sodium chloride | ammonia | aluminum hydroxide formula | NH_4Cl | NaAl(OH)4 | H_2O | NaCl | NH_3 | Al(OH)_3 Hill formula | ClH_4N | H4AlNaO4 | H_2O | ClNa | H_3N | AlH_3O_3 name | ammonium chloride | | water | sodium chloride | ammonia | aluminum hydroxide
| ammonium chloride | NaAl(OH)4 | water | sodium chloride | ammonia | aluminum hydroxide formula | NH_4Cl | NaAl(OH)4 | H_2O | NaCl | NH_3 | Al(OH)_3 Hill formula | ClH_4N | H4AlNaO4 | H_2O | ClNa | H_3N | AlH_3O_3 name | ammonium chloride | | water | sodium chloride | ammonia | aluminum hydroxide

Substance properties

| ammonium chloride | NaAl(OH)4 | water | sodium chloride | ammonia | aluminum hydroxide molar mass | 53.49 g/mol | 118 g/mol | 18.015 g/mol | 58.44 g/mol | 17.031 g/mol | 78.003 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 340 °C | | 0 °C | 801 °C | -77.73 °C | boiling point | | | 99.9839 °C | 1413 °C | -33.33 °C | density | 1.5256 g/cm^3 | | 1 g/cm^3 | 2.16 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | solubility in water | soluble | | | soluble | | surface tension | | | 0.0728 N/m | | 0.0234 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | 1.009×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless | |
| ammonium chloride | NaAl(OH)4 | water | sodium chloride | ammonia | aluminum hydroxide molar mass | 53.49 g/mol | 118 g/mol | 18.015 g/mol | 58.44 g/mol | 17.031 g/mol | 78.003 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 340 °C | | 0 °C | 801 °C | -77.73 °C | boiling point | | | 99.9839 °C | 1413 °C | -33.33 °C | density | 1.5256 g/cm^3 | | 1 g/cm^3 | 2.16 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | solubility in water | soluble | | | soluble | | surface tension | | | 0.0728 N/m | | 0.0234 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | 1.009×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless | |

Units

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