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AgNO3 + AlCl3 = AgCl + Al(NO3)3

Input interpretation

AgNO_3 silver nitrate + AlCl_3 aluminum chloride ⟶ AgCl silver chloride + Al(NO_3)_3 aluminum nitrate
AgNO_3 silver nitrate + AlCl_3 aluminum chloride ⟶ AgCl silver chloride + Al(NO_3)_3 aluminum nitrate

Balanced equation

Balance the chemical equation algebraically: AgNO_3 + AlCl_3 ⟶ AgCl + Al(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 AlCl_3 ⟶ c_3 AgCl + c_4 Al(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Al and Cl: Ag: | c_1 = c_3 N: | c_1 = 3 c_4 O: | 3 c_1 = 9 c_4 Al: | c_2 = c_4 Cl: | 3 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 AgNO_3 + AlCl_3 ⟶ 3 AgCl + Al(NO_3)_3
Balance the chemical equation algebraically: AgNO_3 + AlCl_3 ⟶ AgCl + Al(NO_3)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 AlCl_3 ⟶ c_3 AgCl + c_4 Al(NO_3)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Al and Cl: Ag: | c_1 = c_3 N: | c_1 = 3 c_4 O: | 3 c_1 = 9 c_4 Al: | c_2 = c_4 Cl: | 3 c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 AgNO_3 + AlCl_3 ⟶ 3 AgCl + Al(NO_3)_3

Structures

+ ⟶ +
+ ⟶ +

Names

silver nitrate + aluminum chloride ⟶ silver chloride + aluminum nitrate
silver nitrate + aluminum chloride ⟶ silver chloride + aluminum nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: AgNO_3 + AlCl_3 ⟶ AgCl + Al(NO_3)_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: 3 AgNO_3 + AlCl_3 ⟶ 3 AgCl + Al(NO_3)_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 AgNO_3 | 3 | -3 AlCl_3 | 1 | -1 AgCl | 3 | 3 Al(NO_3)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 3 | -3 | ([AgNO3])^(-3) AlCl_3 | 1 | -1 | ([AlCl3])^(-1) AgCl | 3 | 3 | ([AgCl])^3 Al(NO_3)_3 | 1 | 1 | [Al(NO3)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 = ([AgNO3])^(-3) ([AlCl3])^(-1) ([AgCl])^3 [Al(NO3)3] = (([AgCl])^3 [Al(NO3)3])/(([AgNO3])^3 [AlCl3])
Construct the equilibrium constant, K, expression for: AgNO_3 + AlCl_3 ⟶ AgCl + Al(NO_3)_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: 3 AgNO_3 + AlCl_3 ⟶ 3 AgCl + Al(NO_3)_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 AgNO_3 | 3 | -3 AlCl_3 | 1 | -1 AgCl | 3 | 3 Al(NO_3)_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 3 | -3 | ([AgNO3])^(-3) AlCl_3 | 1 | -1 | ([AlCl3])^(-1) AgCl | 3 | 3 | ([AgCl])^3 Al(NO_3)_3 | 1 | 1 | [Al(NO3)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 = ([AgNO3])^(-3) ([AlCl3])^(-1) ([AgCl])^3 [Al(NO3)3] = (([AgCl])^3 [Al(NO3)3])/(([AgNO3])^3 [AlCl3])

Rate of reaction

Construct the rate of reaction expression for: AgNO_3 + AlCl_3 ⟶ AgCl + Al(NO_3)_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: 3 AgNO_3 + AlCl_3 ⟶ 3 AgCl + Al(NO_3)_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 AgNO_3 | 3 | -3 AlCl_3 | 1 | -1 AgCl | 3 | 3 Al(NO_3)_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 AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) AgCl | 3 | 3 | 1/3 (Δ[AgCl])/(Δt) Al(NO_3)_3 | 1 | 1 | (Δ[Al(NO3)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 = -1/3 (Δ[AgNO3])/(Δt) = -(Δ[AlCl3])/(Δt) = 1/3 (Δ[AgCl])/(Δt) = (Δ[Al(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: AgNO_3 + AlCl_3 ⟶ AgCl + Al(NO_3)_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: 3 AgNO_3 + AlCl_3 ⟶ 3 AgCl + Al(NO_3)_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 AgNO_3 | 3 | -3 AlCl_3 | 1 | -1 AgCl | 3 | 3 Al(NO_3)_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 AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) AgCl | 3 | 3 | 1/3 (Δ[AgCl])/(Δt) Al(NO_3)_3 | 1 | 1 | (Δ[Al(NO3)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 = -1/3 (Δ[AgNO3])/(Δt) = -(Δ[AlCl3])/(Δt) = 1/3 (Δ[AgCl])/(Δt) = (Δ[Al(NO3)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| silver nitrate | aluminum chloride | silver chloride | aluminum nitrate formula | AgNO_3 | AlCl_3 | AgCl | Al(NO_3)_3 Hill formula | AgNO_3 | AlCl_3 | AgCl | AlN_3O_9 name | silver nitrate | aluminum chloride | silver chloride | aluminum nitrate IUPAC name | silver nitrate | trichloroalumane | chlorosilver | aluminum(+3) cation trinitrate
| silver nitrate | aluminum chloride | silver chloride | aluminum nitrate formula | AgNO_3 | AlCl_3 | AgCl | Al(NO_3)_3 Hill formula | AgNO_3 | AlCl_3 | AgCl | AlN_3O_9 name | silver nitrate | aluminum chloride | silver chloride | aluminum nitrate IUPAC name | silver nitrate | trichloroalumane | chlorosilver | aluminum(+3) cation trinitrate

Substance properties

| silver nitrate | aluminum chloride | silver chloride | aluminum nitrate molar mass | 169.87 g/mol | 133.3 g/mol | 143.32 g/mol | 212.99 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 190 °C | 455 °C | 72.8 °C boiling point | | | 1554 °C | density | | | 5.56 g/cm^3 | 1.401 g/cm^3 solubility in water | soluble | | | dynamic viscosity | | | | 0.001338 Pa s (at 22 °C) odor | odorless | | |
| silver nitrate | aluminum chloride | silver chloride | aluminum nitrate molar mass | 169.87 g/mol | 133.3 g/mol | 143.32 g/mol | 212.99 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 190 °C | 455 °C | 72.8 °C boiling point | | | 1554 °C | density | | | 5.56 g/cm^3 | 1.401 g/cm^3 solubility in water | soluble | | | dynamic viscosity | | | | 0.001338 Pa s (at 22 °C) odor | odorless | | |

Units

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