Search

Pb(NO3)2 + AlI3 = Al(NO3)3 + PbI2

Input interpretation

Pb(NO_3)_2 lead(II) nitrate + AlI_3 aluminum iodide ⟶ Al(NO_3)_3 aluminum nitrate + PbI_2 lead iodide
Pb(NO_3)_2 lead(II) nitrate + AlI_3 aluminum iodide ⟶ Al(NO_3)_3 aluminum nitrate + PbI_2 lead iodide

Balanced equation

Balance the chemical equation algebraically: Pb(NO_3)_2 + AlI_3 ⟶ Al(NO_3)_3 + PbI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 AlI_3 ⟶ c_3 Al(NO_3)_3 + c_4 PbI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb, Al and I: N: | 2 c_1 = 3 c_3 O: | 6 c_1 = 9 c_3 Pb: | c_1 = c_4 Al: | c_2 = c_3 I: | 3 c_2 = 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 = 3/2 c_2 = 1 c_3 = 1 c_4 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Pb(NO_3)_2 + 2 AlI_3 ⟶ 2 Al(NO_3)_3 + 3 PbI_2
Balance the chemical equation algebraically: Pb(NO_3)_2 + AlI_3 ⟶ Al(NO_3)_3 + PbI_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 AlI_3 ⟶ c_3 Al(NO_3)_3 + c_4 PbI_2 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb, Al and I: N: | 2 c_1 = 3 c_3 O: | 6 c_1 = 9 c_3 Pb: | c_1 = c_4 Al: | c_2 = c_3 I: | 3 c_2 = 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 = 3/2 c_2 = 1 c_3 = 1 c_4 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 2 c_4 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Pb(NO_3)_2 + 2 AlI_3 ⟶ 2 Al(NO_3)_3 + 3 PbI_2

Structures

+ ⟶ +
+ ⟶ +

Names

lead(II) nitrate + aluminum iodide ⟶ aluminum nitrate + lead iodide
lead(II) nitrate + aluminum iodide ⟶ aluminum nitrate + lead iodide

Equilibrium constant

Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + AlI_3 ⟶ Al(NO_3)_3 + PbI_2 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 Pb(NO_3)_2 + 2 AlI_3 ⟶ 2 Al(NO_3)_3 + 3 PbI_2 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 Pb(NO_3)_2 | 3 | -3 AlI_3 | 2 | -2 Al(NO_3)_3 | 2 | 2 PbI_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Pb(NO_3)_2 | 3 | -3 | ([Pb(NO3)2])^(-3) AlI_3 | 2 | -2 | ([AlI3])^(-2) Al(NO_3)_3 | 2 | 2 | ([Al(NO3)3])^2 PbI_2 | 3 | 3 | ([PbI2])^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 = ([Pb(NO3)2])^(-3) ([AlI3])^(-2) ([Al(NO3)3])^2 ([PbI2])^3 = (([Al(NO3)3])^2 ([PbI2])^3)/(([Pb(NO3)2])^3 ([AlI3])^2)
Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + AlI_3 ⟶ Al(NO_3)_3 + PbI_2 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 Pb(NO_3)_2 + 2 AlI_3 ⟶ 2 Al(NO_3)_3 + 3 PbI_2 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 Pb(NO_3)_2 | 3 | -3 AlI_3 | 2 | -2 Al(NO_3)_3 | 2 | 2 PbI_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Pb(NO_3)_2 | 3 | -3 | ([Pb(NO3)2])^(-3) AlI_3 | 2 | -2 | ([AlI3])^(-2) Al(NO_3)_3 | 2 | 2 | ([Al(NO3)3])^2 PbI_2 | 3 | 3 | ([PbI2])^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 = ([Pb(NO3)2])^(-3) ([AlI3])^(-2) ([Al(NO3)3])^2 ([PbI2])^3 = (([Al(NO3)3])^2 ([PbI2])^3)/(([Pb(NO3)2])^3 ([AlI3])^2)

Rate of reaction

Construct the rate of reaction expression for: Pb(NO_3)_2 + AlI_3 ⟶ Al(NO_3)_3 + PbI_2 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 Pb(NO_3)_2 + 2 AlI_3 ⟶ 2 Al(NO_3)_3 + 3 PbI_2 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 Pb(NO_3)_2 | 3 | -3 AlI_3 | 2 | -2 Al(NO_3)_3 | 2 | 2 PbI_2 | 3 | 3 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 Pb(NO_3)_2 | 3 | -3 | -1/3 (Δ[Pb(NO3)2])/(Δt) AlI_3 | 2 | -2 | -1/2 (Δ[AlI3])/(Δt) Al(NO_3)_3 | 2 | 2 | 1/2 (Δ[Al(NO3)3])/(Δt) PbI_2 | 3 | 3 | 1/3 (Δ[PbI2])/(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[Pb(NO3)2])/(Δt) = -1/2 (Δ[AlI3])/(Δt) = 1/2 (Δ[Al(NO3)3])/(Δt) = 1/3 (Δ[PbI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Pb(NO_3)_2 + AlI_3 ⟶ Al(NO_3)_3 + PbI_2 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 Pb(NO_3)_2 + 2 AlI_3 ⟶ 2 Al(NO_3)_3 + 3 PbI_2 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 Pb(NO_3)_2 | 3 | -3 AlI_3 | 2 | -2 Al(NO_3)_3 | 2 | 2 PbI_2 | 3 | 3 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 Pb(NO_3)_2 | 3 | -3 | -1/3 (Δ[Pb(NO3)2])/(Δt) AlI_3 | 2 | -2 | -1/2 (Δ[AlI3])/(Δt) Al(NO_3)_3 | 2 | 2 | 1/2 (Δ[Al(NO3)3])/(Δt) PbI_2 | 3 | 3 | 1/3 (Δ[PbI2])/(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[Pb(NO3)2])/(Δt) = -1/2 (Δ[AlI3])/(Δt) = 1/2 (Δ[Al(NO3)3])/(Δt) = 1/3 (Δ[PbI2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| lead(II) nitrate | aluminum iodide | aluminum nitrate | lead iodide formula | Pb(NO_3)_2 | AlI_3 | Al(NO_3)_3 | PbI_2 Hill formula | N_2O_6Pb | AlI_3 | AlN_3O_9 | I_2Pb name | lead(II) nitrate | aluminum iodide | aluminum nitrate | lead iodide IUPAC name | plumbous dinitrate | triiodoalumane | aluminum(+3) cation trinitrate |
| lead(II) nitrate | aluminum iodide | aluminum nitrate | lead iodide formula | Pb(NO_3)_2 | AlI_3 | Al(NO_3)_3 | PbI_2 Hill formula | N_2O_6Pb | AlI_3 | AlN_3O_9 | I_2Pb name | lead(II) nitrate | aluminum iodide | aluminum nitrate | lead iodide IUPAC name | plumbous dinitrate | triiodoalumane | aluminum(+3) cation trinitrate |

Substance properties

| lead(II) nitrate | aluminum iodide | aluminum nitrate | lead iodide molar mass | 331.2 g/mol | 407.69495 g/mol | 212.99 g/mol | 461 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 191 °C | 72.8 °C | 402 °C boiling point | | 360 °C | | 954 °C density | | 3.98 g/cm^3 | 1.401 g/cm^3 | 6.16 g/cm^3 solubility in water | | decomposes | | dynamic viscosity | | | 0.001338 Pa s (at 22 °C) | odor | odorless | | |
| lead(II) nitrate | aluminum iodide | aluminum nitrate | lead iodide molar mass | 331.2 g/mol | 407.69495 g/mol | 212.99 g/mol | 461 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 191 °C | 72.8 °C | 402 °C boiling point | | 360 °C | | 954 °C density | | 3.98 g/cm^3 | 1.401 g/cm^3 | 6.16 g/cm^3 solubility in water | | decomposes | | dynamic viscosity | | | 0.001338 Pa s (at 22 °C) | odor | odorless | | |

Units

Random Queries

IUPAC name of N-(tert-butoxycarbonyl)-D-prolinal vs 1-benzyl-4-(N-boc-amino)piperidine
molecules per unit cell of corundum vs downeyite
handwritten style O2 vs N2 vs CO2
dimercury(I) cation vs oxide anion
formula string of indium(III) cation
formula of 2-amino-2-deoxy-isochorismate
chemical uses of benzene
disodium hydrogen phosphate vs 1-ethylquinaldinium iodide
Br2 + P = PBr
first ionization energy of zinc