Input interpretation
![Pb(NO_3)_2 lead(II) nitrate + Ni nickel ⟶ Pb lead + Ni(NO_3)_2 nickel(II) nitrate](../image_source/ae55fb43446aec8d4e766ef7abe44ba5.png)
Pb(NO_3)_2 lead(II) nitrate + Ni nickel ⟶ Pb lead + Ni(NO_3)_2 nickel(II) nitrate
Balanced equation
![Balance the chemical equation algebraically: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 Ni ⟶ c_3 Pb + c_4 Ni(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb and Ni: N: | 2 c_1 = 2 c_4 O: | 6 c_1 = 6 c_4 Pb: | c_1 = c_3 Ni: | 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_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: | | Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_2](../image_source/5000954e8a51b4350316b7a475e98988.png)
Balance the chemical equation algebraically: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 Ni ⟶ c_3 Pb + c_4 Ni(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb and Ni: N: | 2 c_1 = 2 c_4 O: | 6 c_1 = 6 c_4 Pb: | c_1 = c_3 Ni: | 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_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: | | Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_2
Structures
![+ ⟶ +](../image_source/ebad0298fd0b2a3bbab3dfd9d1195b3f.png)
+ ⟶ +
Names
![lead(II) nitrate + nickel ⟶ lead + nickel(II) nitrate](../image_source/077ec9c9c20a33da97485e987c9c8d04.png)
lead(II) nitrate + nickel ⟶ lead + nickel(II) nitrate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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 | 1 | -1 Ni | 1 | -1 Pb | 1 | 1 Ni(NO_3)_2 | 1 | 1 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 | 1 | -1 | ([Pb(NO3)2])^(-1) Ni | 1 | -1 | ([Ni])^(-1) Pb | 1 | 1 | [Pb] Ni(NO_3)_2 | 1 | 1 | [Ni(NO3)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 = ([Pb(NO3)2])^(-1) ([Ni])^(-1) [Pb] [Ni(NO3)2] = ([Pb] [Ni(NO3)2])/([Pb(NO3)2] [Ni])](../image_source/facff45e824f363d43a4ee56baa973c7.png)
Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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 | 1 | -1 Ni | 1 | -1 Pb | 1 | 1 Ni(NO_3)_2 | 1 | 1 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 | 1 | -1 | ([Pb(NO3)2])^(-1) Ni | 1 | -1 | ([Ni])^(-1) Pb | 1 | 1 | [Pb] Ni(NO_3)_2 | 1 | 1 | [Ni(NO3)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 = ([Pb(NO3)2])^(-1) ([Ni])^(-1) [Pb] [Ni(NO3)2] = ([Pb] [Ni(NO3)2])/([Pb(NO3)2] [Ni])
Rate of reaction
![Construct the rate of reaction expression for: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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 | 1 | -1 Ni | 1 | -1 Pb | 1 | 1 Ni(NO_3)_2 | 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 Pb(NO_3)_2 | 1 | -1 | -(Δ[Pb(NO3)2])/(Δt) Ni | 1 | -1 | -(Δ[Ni])/(Δt) Pb | 1 | 1 | (Δ[Pb])/(Δt) Ni(NO_3)_2 | 1 | 1 | (Δ[Ni(NO3)2])/(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[Pb(NO3)2])/(Δt) = -(Δ[Ni])/(Δt) = (Δ[Pb])/(Δt) = (Δ[Ni(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/4f495ab4ecf54dfab883f171533070ab.png)
Construct the rate of reaction expression for: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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: Pb(NO_3)_2 + Ni ⟶ Pb + Ni(NO_3)_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 | 1 | -1 Ni | 1 | -1 Pb | 1 | 1 Ni(NO_3)_2 | 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 Pb(NO_3)_2 | 1 | -1 | -(Δ[Pb(NO3)2])/(Δt) Ni | 1 | -1 | -(Δ[Ni])/(Δt) Pb | 1 | 1 | (Δ[Pb])/(Δt) Ni(NO_3)_2 | 1 | 1 | (Δ[Ni(NO3)2])/(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[Pb(NO3)2])/(Δt) = -(Δ[Ni])/(Δt) = (Δ[Pb])/(Δt) = (Δ[Ni(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| lead(II) nitrate | nickel | lead | nickel(II) nitrate formula | Pb(NO_3)_2 | Ni | Pb | Ni(NO_3)_2 Hill formula | N_2O_6Pb | Ni | Pb | N_2NiO_6 name | lead(II) nitrate | nickel | lead | nickel(II) nitrate IUPAC name | plumbous dinitrate | nickel | lead | nickel(+2) dinitrate](../image_source/b65e0193fea289479606550d89748850.png)
| lead(II) nitrate | nickel | lead | nickel(II) nitrate formula | Pb(NO_3)_2 | Ni | Pb | Ni(NO_3)_2 Hill formula | N_2O_6Pb | Ni | Pb | N_2NiO_6 name | lead(II) nitrate | nickel | lead | nickel(II) nitrate IUPAC name | plumbous dinitrate | nickel | lead | nickel(+2) dinitrate
Substance properties
![| lead(II) nitrate | nickel | lead | nickel(II) nitrate molar mass | 331.2 g/mol | 58.6934 g/mol | 207.2 g/mol | 182.7 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 1453 °C | 327.4 °C | 57 °C boiling point | | 2732 °C | 1740 °C | 137 °C density | | 8.908 g/cm^3 | 11.34 g/cm^3 | 1.77 g/cm^3 solubility in water | | insoluble | insoluble | dynamic viscosity | | | 0.00183 Pa s (at 38 °C) | odor | odorless | odorless | |](../image_source/ae2b0ff095627800b2ebd940a4158ae4.png)
| lead(II) nitrate | nickel | lead | nickel(II) nitrate molar mass | 331.2 g/mol | 58.6934 g/mol | 207.2 g/mol | 182.7 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 1453 °C | 327.4 °C | 57 °C boiling point | | 2732 °C | 1740 °C | 137 °C density | | 8.908 g/cm^3 | 11.34 g/cm^3 | 1.77 g/cm^3 solubility in water | | insoluble | insoluble | dynamic viscosity | | | 0.00183 Pa s (at 38 °C) | odor | odorless | odorless | |
Units