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NaOH + PbO2 + NaCrO2 = H2O + Na2CrO4 + NaPbO2

Input interpretation

NaOH sodium hydroxide + PbO_2 lead dioxide + NaCrO2 ⟶ H_2O water + Na_2CrO_4 sodium chromate + NaPbO2
NaOH sodium hydroxide + PbO_2 lead dioxide + NaCrO2 ⟶ H_2O water + Na_2CrO_4 sodium chromate + NaPbO2

Balanced equation

Balance the chemical equation algebraically: NaOH + PbO_2 + NaCrO2 ⟶ H_2O + Na_2CrO_4 + NaPbO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 PbO_2 + c_3 NaCrO2 ⟶ c_4 H_2O + c_5 Na_2CrO_4 + c_6 NaPbO2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Pb and Cr: H: | c_1 = 2 c_4 Na: | c_1 + c_3 = 2 c_5 + c_6 O: | c_1 + 2 c_2 + 2 c_3 = c_4 + 4 c_5 + 2 c_6 Pb: | c_2 = c_6 Cr: | c_3 = c_5 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + 3 PbO_2 + NaCrO2 ⟶ 2 H_2O + Na_2CrO_4 + 3 NaPbO2
Balance the chemical equation algebraically: NaOH + PbO_2 + NaCrO2 ⟶ H_2O + Na_2CrO_4 + NaPbO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 PbO_2 + c_3 NaCrO2 ⟶ c_4 H_2O + c_5 Na_2CrO_4 + c_6 NaPbO2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Pb and Cr: H: | c_1 = 2 c_4 Na: | c_1 + c_3 = 2 c_5 + c_6 O: | c_1 + 2 c_2 + 2 c_3 = c_4 + 4 c_5 + 2 c_6 Pb: | c_2 = c_6 Cr: | c_3 = c_5 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + 3 PbO_2 + NaCrO2 ⟶ 2 H_2O + Na_2CrO_4 + 3 NaPbO2

Structures

+ + NaCrO2 ⟶ + + NaPbO2
+ + NaCrO2 ⟶ + + NaPbO2

Names

sodium hydroxide + lead dioxide + NaCrO2 ⟶ water + sodium chromate + NaPbO2
sodium hydroxide + lead dioxide + NaCrO2 ⟶ water + sodium chromate + NaPbO2

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + PbO_2 + NaCrO2 ⟶ H_2O + Na_2CrO_4 + NaPbO2 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: 4 NaOH + 3 PbO_2 + NaCrO2 ⟶ 2 H_2O + Na_2CrO_4 + 3 NaPbO2 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 NaOH | 4 | -4 PbO_2 | 3 | -3 NaCrO2 | 1 | -1 H_2O | 2 | 2 Na_2CrO_4 | 1 | 1 NaPbO2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 4 | -4 | ([NaOH])^(-4) PbO_2 | 3 | -3 | ([PbO2])^(-3) NaCrO2 | 1 | -1 | ([NaCrO2])^(-1) H_2O | 2 | 2 | ([H2O])^2 Na_2CrO_4 | 1 | 1 | [Na2CrO4] NaPbO2 | 3 | 3 | ([NaPbO2])^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 = ([NaOH])^(-4) ([PbO2])^(-3) ([NaCrO2])^(-1) ([H2O])^2 [Na2CrO4] ([NaPbO2])^3 = (([H2O])^2 [Na2CrO4] ([NaPbO2])^3)/(([NaOH])^4 ([PbO2])^3 [NaCrO2])
Construct the equilibrium constant, K, expression for: NaOH + PbO_2 + NaCrO2 ⟶ H_2O + Na_2CrO_4 + NaPbO2 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: 4 NaOH + 3 PbO_2 + NaCrO2 ⟶ 2 H_2O + Na_2CrO_4 + 3 NaPbO2 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 NaOH | 4 | -4 PbO_2 | 3 | -3 NaCrO2 | 1 | -1 H_2O | 2 | 2 Na_2CrO_4 | 1 | 1 NaPbO2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 4 | -4 | ([NaOH])^(-4) PbO_2 | 3 | -3 | ([PbO2])^(-3) NaCrO2 | 1 | -1 | ([NaCrO2])^(-1) H_2O | 2 | 2 | ([H2O])^2 Na_2CrO_4 | 1 | 1 | [Na2CrO4] NaPbO2 | 3 | 3 | ([NaPbO2])^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 = ([NaOH])^(-4) ([PbO2])^(-3) ([NaCrO2])^(-1) ([H2O])^2 [Na2CrO4] ([NaPbO2])^3 = (([H2O])^2 [Na2CrO4] ([NaPbO2])^3)/(([NaOH])^4 ([PbO2])^3 [NaCrO2])

Rate of reaction

Construct the rate of reaction expression for: NaOH + PbO_2 + NaCrO2 ⟶ H_2O + Na_2CrO_4 + NaPbO2 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: 4 NaOH + 3 PbO_2 + NaCrO2 ⟶ 2 H_2O + Na_2CrO_4 + 3 NaPbO2 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 NaOH | 4 | -4 PbO_2 | 3 | -3 NaCrO2 | 1 | -1 H_2O | 2 | 2 Na_2CrO_4 | 1 | 1 NaPbO2 | 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 NaOH | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) PbO_2 | 3 | -3 | -1/3 (Δ[PbO2])/(Δt) NaCrO2 | 1 | -1 | -(Δ[NaCrO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Na_2CrO_4 | 1 | 1 | (Δ[Na2CrO4])/(Δt) NaPbO2 | 3 | 3 | 1/3 (Δ[NaPbO2])/(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 = -1/4 (Δ[NaOH])/(Δt) = -1/3 (Δ[PbO2])/(Δt) = -(Δ[NaCrO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[Na2CrO4])/(Δt) = 1/3 (Δ[NaPbO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + PbO_2 + NaCrO2 ⟶ H_2O + Na_2CrO_4 + NaPbO2 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: 4 NaOH + 3 PbO_2 + NaCrO2 ⟶ 2 H_2O + Na_2CrO_4 + 3 NaPbO2 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 NaOH | 4 | -4 PbO_2 | 3 | -3 NaCrO2 | 1 | -1 H_2O | 2 | 2 Na_2CrO_4 | 1 | 1 NaPbO2 | 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 NaOH | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) PbO_2 | 3 | -3 | -1/3 (Δ[PbO2])/(Δt) NaCrO2 | 1 | -1 | -(Δ[NaCrO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Na_2CrO_4 | 1 | 1 | (Δ[Na2CrO4])/(Δt) NaPbO2 | 3 | 3 | 1/3 (Δ[NaPbO2])/(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 = -1/4 (Δ[NaOH])/(Δt) = -1/3 (Δ[PbO2])/(Δt) = -(Δ[NaCrO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[Na2CrO4])/(Δt) = 1/3 (Δ[NaPbO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | lead dioxide | NaCrO2 | water | sodium chromate | NaPbO2 formula | NaOH | PbO_2 | NaCrO2 | H_2O | Na_2CrO_4 | NaPbO2 Hill formula | HNaO | O_2Pb | CrNaO2 | H_2O | CrNa_2O_4 | NaO2Pb name | sodium hydroxide | lead dioxide | | water | sodium chromate | IUPAC name | sodium hydroxide | | | water | disodium dioxido(dioxo)chromium |
| sodium hydroxide | lead dioxide | NaCrO2 | water | sodium chromate | NaPbO2 formula | NaOH | PbO_2 | NaCrO2 | H_2O | Na_2CrO_4 | NaPbO2 Hill formula | HNaO | O_2Pb | CrNaO2 | H_2O | CrNa_2O_4 | NaO2Pb name | sodium hydroxide | lead dioxide | | water | sodium chromate | IUPAC name | sodium hydroxide | | | water | disodium dioxido(dioxo)chromium |

Substance properties

| sodium hydroxide | lead dioxide | NaCrO2 | water | sodium chromate | NaPbO2 molar mass | 39.997 g/mol | 239.2 g/mol | 106.98 g/mol | 18.015 g/mol | 161.97 g/mol | 262.2 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | melting point | 323 °C | 290 °C | | 0 °C | 780 °C | boiling point | 1390 °C | | | 99.9839 °C | | density | 2.13 g/cm^3 | 9.58 g/cm^3 | | 1 g/cm^3 | 2.698 g/cm^3 | solubility in water | soluble | insoluble | | | | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | |
| sodium hydroxide | lead dioxide | NaCrO2 | water | sodium chromate | NaPbO2 molar mass | 39.997 g/mol | 239.2 g/mol | 106.98 g/mol | 18.015 g/mol | 161.97 g/mol | 262.2 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | melting point | 323 °C | 290 °C | | 0 °C | 780 °C | boiling point | 1390 °C | | | 99.9839 °C | | density | 2.13 g/cm^3 | 9.58 g/cm^3 | | 1 g/cm^3 | 2.698 g/cm^3 | solubility in water | soluble | insoluble | | | | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | |

Units

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