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Pb(NO3)2 + Na2CrO4 = NaNO3 + PbCrO4

Input interpretation

Pb(NO_3)_2 lead(II) nitrate + Na_2CrO_4 sodium chromate ⟶ NaNO_3 sodium nitrate + PbCrO_4 lead(II) chromate
Pb(NO_3)_2 lead(II) nitrate + Na_2CrO_4 sodium chromate ⟶ NaNO_3 sodium nitrate + PbCrO_4 lead(II) chromate

Balanced equation

Balance the chemical equation algebraically: Pb(NO_3)_2 + Na_2CrO_4 ⟶ NaNO_3 + PbCrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 Na_2CrO_4 ⟶ c_3 NaNO_3 + c_4 PbCrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb, Cr and Na: N: | 2 c_1 = c_3 O: | 6 c_1 + 4 c_2 = 3 c_3 + 4 c_4 Pb: | c_1 = c_4 Cr: | c_2 = c_4 Na: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Pb(NO_3)_2 + Na_2CrO_4 ⟶ 2 NaNO_3 + PbCrO_4
Balance the chemical equation algebraically: Pb(NO_3)_2 + Na_2CrO_4 ⟶ NaNO_3 + PbCrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Pb(NO_3)_2 + c_2 Na_2CrO_4 ⟶ c_3 NaNO_3 + c_4 PbCrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O, Pb, Cr and Na: N: | 2 c_1 = c_3 O: | 6 c_1 + 4 c_2 = 3 c_3 + 4 c_4 Pb: | c_1 = c_4 Cr: | c_2 = c_4 Na: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Pb(NO_3)_2 + Na_2CrO_4 ⟶ 2 NaNO_3 + PbCrO_4

Structures

+ ⟶ +
+ ⟶ +

Names

lead(II) nitrate + sodium chromate ⟶ sodium nitrate + lead(II) chromate
lead(II) nitrate + sodium chromate ⟶ sodium nitrate + lead(II) chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + Na_2CrO_4 ⟶ NaNO_3 + PbCrO_4 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 + Na_2CrO_4 ⟶ 2 NaNO_3 + PbCrO_4 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 Na_2CrO_4 | 1 | -1 NaNO_3 | 2 | 2 PbCrO_4 | 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) Na_2CrO_4 | 1 | -1 | ([Na2CrO4])^(-1) NaNO_3 | 2 | 2 | ([NaNO3])^2 PbCrO_4 | 1 | 1 | [PbCrO4] 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) ([Na2CrO4])^(-1) ([NaNO3])^2 [PbCrO4] = (([NaNO3])^2 [PbCrO4])/([Pb(NO3)2] [Na2CrO4])
Construct the equilibrium constant, K, expression for: Pb(NO_3)_2 + Na_2CrO_4 ⟶ NaNO_3 + PbCrO_4 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 + Na_2CrO_4 ⟶ 2 NaNO_3 + PbCrO_4 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 Na_2CrO_4 | 1 | -1 NaNO_3 | 2 | 2 PbCrO_4 | 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) Na_2CrO_4 | 1 | -1 | ([Na2CrO4])^(-1) NaNO_3 | 2 | 2 | ([NaNO3])^2 PbCrO_4 | 1 | 1 | [PbCrO4] 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) ([Na2CrO4])^(-1) ([NaNO3])^2 [PbCrO4] = (([NaNO3])^2 [PbCrO4])/([Pb(NO3)2] [Na2CrO4])

Rate of reaction

Construct the rate of reaction expression for: Pb(NO_3)_2 + Na_2CrO_4 ⟶ NaNO_3 + PbCrO_4 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 + Na_2CrO_4 ⟶ 2 NaNO_3 + PbCrO_4 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 Na_2CrO_4 | 1 | -1 NaNO_3 | 2 | 2 PbCrO_4 | 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) Na_2CrO_4 | 1 | -1 | -(Δ[Na2CrO4])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) PbCrO_4 | 1 | 1 | (Δ[PbCrO4])/(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[Na2CrO4])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = (Δ[PbCrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Pb(NO_3)_2 + Na_2CrO_4 ⟶ NaNO_3 + PbCrO_4 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 + Na_2CrO_4 ⟶ 2 NaNO_3 + PbCrO_4 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 Na_2CrO_4 | 1 | -1 NaNO_3 | 2 | 2 PbCrO_4 | 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) Na_2CrO_4 | 1 | -1 | -(Δ[Na2CrO4])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) PbCrO_4 | 1 | 1 | (Δ[PbCrO4])/(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[Na2CrO4])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = (Δ[PbCrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| lead(II) nitrate | sodium chromate | sodium nitrate | lead(II) chromate formula | Pb(NO_3)_2 | Na_2CrO_4 | NaNO_3 | PbCrO_4 Hill formula | N_2O_6Pb | CrNa_2O_4 | NNaO_3 | CrO_4Pb name | lead(II) nitrate | sodium chromate | sodium nitrate | lead(II) chromate IUPAC name | plumbous dinitrate | disodium dioxido(dioxo)chromium | sodium nitrate | plumbous dioxido-dioxochromium
| lead(II) nitrate | sodium chromate | sodium nitrate | lead(II) chromate formula | Pb(NO_3)_2 | Na_2CrO_4 | NaNO_3 | PbCrO_4 Hill formula | N_2O_6Pb | CrNa_2O_4 | NNaO_3 | CrO_4Pb name | lead(II) nitrate | sodium chromate | sodium nitrate | lead(II) chromate IUPAC name | plumbous dinitrate | disodium dioxido(dioxo)chromium | sodium nitrate | plumbous dioxido-dioxochromium

Substance properties

| lead(II) nitrate | sodium chromate | sodium nitrate | lead(II) chromate molar mass | 331.2 g/mol | 161.97 g/mol | 84.994 g/mol | 323.2 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 780 °C | 306 °C | 844 °C density | | 2.698 g/cm^3 | 2.26 g/cm^3 | 6.023 g/cm^3 solubility in water | | | soluble | dynamic viscosity | | | 0.003 Pa s (at 250 °C) | odor | odorless | | |
| lead(II) nitrate | sodium chromate | sodium nitrate | lead(II) chromate molar mass | 331.2 g/mol | 161.97 g/mol | 84.994 g/mol | 323.2 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 470 °C | 780 °C | 306 °C | 844 °C density | | 2.698 g/cm^3 | 2.26 g/cm^3 | 6.023 g/cm^3 solubility in water | | | soluble | dynamic viscosity | | | 0.003 Pa s (at 250 °C) | odor | odorless | | |

Units

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