Search

H2O + PbO2 = O2 + Pb(OH)2

Input interpretation

H_2O water + PbO_2 lead dioxide ⟶ O_2 oxygen + Pb(OH)_2 lead(II) hydroxide
H_2O water + PbO_2 lead dioxide ⟶ O_2 oxygen + Pb(OH)_2 lead(II) hydroxide

Balanced equation

Balance the chemical equation algebraically: H_2O + PbO_2 ⟶ O_2 + Pb(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 PbO_2 ⟶ c_3 O_2 + c_4 Pb(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Pb: H: | 2 c_1 = 2 c_4 O: | c_1 + 2 c_2 = 2 c_3 + 2 c_4 Pb: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 PbO_2 ⟶ O_2 + 2 Pb(OH)_2
Balance the chemical equation algebraically: H_2O + PbO_2 ⟶ O_2 + Pb(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 PbO_2 ⟶ c_3 O_2 + c_4 Pb(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Pb: H: | 2 c_1 = 2 c_4 O: | c_1 + 2 c_2 = 2 c_3 + 2 c_4 Pb: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 PbO_2 ⟶ O_2 + 2 Pb(OH)_2

Structures

+ ⟶ +
+ ⟶ +

Names

water + lead dioxide ⟶ oxygen + lead(II) hydroxide
water + lead dioxide ⟶ oxygen + lead(II) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + PbO_2 ⟶ O_2 + Pb(OH)_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: 2 H_2O + 2 PbO_2 ⟶ O_2 + 2 Pb(OH)_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 H_2O | 2 | -2 PbO_2 | 2 | -2 O_2 | 1 | 1 Pb(OH)_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) PbO_2 | 2 | -2 | ([PbO2])^(-2) O_2 | 1 | 1 | [O2] Pb(OH)_2 | 2 | 2 | ([Pb(OH)2])^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 = ([H2O])^(-2) ([PbO2])^(-2) [O2] ([Pb(OH)2])^2 = ([O2] ([Pb(OH)2])^2)/(([H2O])^2 ([PbO2])^2)
Construct the equilibrium constant, K, expression for: H_2O + PbO_2 ⟶ O_2 + Pb(OH)_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: 2 H_2O + 2 PbO_2 ⟶ O_2 + 2 Pb(OH)_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 H_2O | 2 | -2 PbO_2 | 2 | -2 O_2 | 1 | 1 Pb(OH)_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) PbO_2 | 2 | -2 | ([PbO2])^(-2) O_2 | 1 | 1 | [O2] Pb(OH)_2 | 2 | 2 | ([Pb(OH)2])^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 = ([H2O])^(-2) ([PbO2])^(-2) [O2] ([Pb(OH)2])^2 = ([O2] ([Pb(OH)2])^2)/(([H2O])^2 ([PbO2])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2O + PbO_2 ⟶ O_2 + Pb(OH)_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: 2 H_2O + 2 PbO_2 ⟶ O_2 + 2 Pb(OH)_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 H_2O | 2 | -2 PbO_2 | 2 | -2 O_2 | 1 | 1 Pb(OH)_2 | 2 | 2 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) PbO_2 | 2 | -2 | -1/2 (Δ[PbO2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Pb(OH)_2 | 2 | 2 | 1/2 (Δ[Pb(OH)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 = -1/2 (Δ[H2O])/(Δt) = -1/2 (Δ[PbO2])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[Pb(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + PbO_2 ⟶ O_2 + Pb(OH)_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: 2 H_2O + 2 PbO_2 ⟶ O_2 + 2 Pb(OH)_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 H_2O | 2 | -2 PbO_2 | 2 | -2 O_2 | 1 | 1 Pb(OH)_2 | 2 | 2 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) PbO_2 | 2 | -2 | -1/2 (Δ[PbO2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Pb(OH)_2 | 2 | 2 | 1/2 (Δ[Pb(OH)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 = -1/2 (Δ[H2O])/(Δt) = -1/2 (Δ[PbO2])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[Pb(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | lead dioxide | oxygen | lead(II) hydroxide formula | H_2O | PbO_2 | O_2 | Pb(OH)_2 Hill formula | H_2O | O_2Pb | O_2 | H_2O_2Pb name | water | lead dioxide | oxygen | lead(II) hydroxide IUPAC name | water | | molecular oxygen | plumbous dihydroxide
| water | lead dioxide | oxygen | lead(II) hydroxide formula | H_2O | PbO_2 | O_2 | Pb(OH)_2 Hill formula | H_2O | O_2Pb | O_2 | H_2O_2Pb name | water | lead dioxide | oxygen | lead(II) hydroxide IUPAC name | water | | molecular oxygen | plumbous dihydroxide

Substance properties

| water | lead dioxide | oxygen | lead(II) hydroxide molar mass | 18.015 g/mol | 239.2 g/mol | 31.998 g/mol | 241.2 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 0 °C | 290 °C | -218 °C | boiling point | 99.9839 °C | | -183 °C | density | 1 g/cm^3 | 9.58 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | solubility in water | | insoluble | | surface tension | 0.0728 N/m | | 0.01347 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 2.055×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless |
| water | lead dioxide | oxygen | lead(II) hydroxide molar mass | 18.015 g/mol | 239.2 g/mol | 31.998 g/mol | 241.2 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | melting point | 0 °C | 290 °C | -218 °C | boiling point | 99.9839 °C | | -183 °C | density | 1 g/cm^3 | 9.58 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | solubility in water | | insoluble | | surface tension | 0.0728 N/m | | 0.01347 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 2.055×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless |

Units

Random Queries

cobalt monoxide
molar mass of lead(II) nitrate vs lithium molybdate
alternate names of sodium arsenate vs calcium oxalate hydrate
structure diagram of palladium(IV) cation vs zinc cation
alternate names of sodium metatitanate
alternate names of sodium metavanadate
formula of sodium amide vs nitric acid
formula of cadmium carbonate
molar mass of magnesium perborate heptahydrate vs sodium permanganate
molar mass of sodium aluminate vs ammonium tetrachloroaurate(III) hydrate