Search

H2O + NaClO + Pb(CH3COO)2 = NaCl + CH3COOH + PbO2

Input interpretation

H_2O water + NaOCl sodium hypochlorite + Pb(CH_3CO_2)_2 lead(II) acetate ⟶ NaCl sodium chloride + CH_3CO_2H acetic acid + PbO_2 lead dioxide
H_2O water + NaOCl sodium hypochlorite + Pb(CH_3CO_2)_2 lead(II) acetate ⟶ NaCl sodium chloride + CH_3CO_2H acetic acid + PbO_2 lead dioxide

Balanced equation

Balance the chemical equation algebraically: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + CH_3CO_2H + PbO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NaOCl + c_3 Pb(CH_3CO_2)_2 ⟶ c_4 NaCl + c_5 CH_3CO_2H + c_6 PbO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Na, C and Pb: H: | 2 c_1 + 6 c_3 = 4 c_5 O: | c_1 + c_2 + 4 c_3 = 2 c_5 + 2 c_6 Cl: | c_2 = c_4 Na: | c_2 = c_4 C: | 4 c_3 = 2 c_5 Pb: | c_3 = c_6 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 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + 2 CH_3CO_2H + PbO_2
Balance the chemical equation algebraically: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + CH_3CO_2H + PbO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NaOCl + c_3 Pb(CH_3CO_2)_2 ⟶ c_4 NaCl + c_5 CH_3CO_2H + c_6 PbO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Na, C and Pb: H: | 2 c_1 + 6 c_3 = 4 c_5 O: | c_1 + c_2 + 4 c_3 = 2 c_5 + 2 c_6 Cl: | c_2 = c_4 Na: | c_2 = c_4 C: | 4 c_3 = 2 c_5 Pb: | c_3 = c_6 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 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + 2 CH_3CO_2H + PbO_2

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + sodium hypochlorite + lead(II) acetate ⟶ sodium chloride + acetic acid + lead dioxide
water + sodium hypochlorite + lead(II) acetate ⟶ sodium chloride + acetic acid + lead dioxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + CH_3CO_2H + PbO_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: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + 2 CH_3CO_2H + PbO_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 | 1 | -1 NaOCl | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 NaCl | 1 | 1 CH_3CO_2H | 2 | 2 PbO_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) NaOCl | 1 | -1 | ([NaOCl])^(-1) Pb(CH_3CO_2)_2 | 1 | -1 | ([Pb(CH3CO2)2])^(-1) NaCl | 1 | 1 | [NaCl] CH_3CO_2H | 2 | 2 | ([CH3CO2H])^2 PbO_2 | 1 | 1 | [PbO2] 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])^(-1) ([NaOCl])^(-1) ([Pb(CH3CO2)2])^(-1) [NaCl] ([CH3CO2H])^2 [PbO2] = ([NaCl] ([CH3CO2H])^2 [PbO2])/([H2O] [NaOCl] [Pb(CH3CO2)2])
Construct the equilibrium constant, K, expression for: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + CH_3CO_2H + PbO_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: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + 2 CH_3CO_2H + PbO_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 | 1 | -1 NaOCl | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 NaCl | 1 | 1 CH_3CO_2H | 2 | 2 PbO_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) NaOCl | 1 | -1 | ([NaOCl])^(-1) Pb(CH_3CO_2)_2 | 1 | -1 | ([Pb(CH3CO2)2])^(-1) NaCl | 1 | 1 | [NaCl] CH_3CO_2H | 2 | 2 | ([CH3CO2H])^2 PbO_2 | 1 | 1 | [PbO2] 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])^(-1) ([NaOCl])^(-1) ([Pb(CH3CO2)2])^(-1) [NaCl] ([CH3CO2H])^2 [PbO2] = ([NaCl] ([CH3CO2H])^2 [PbO2])/([H2O] [NaOCl] [Pb(CH3CO2)2])

Rate of reaction

Construct the rate of reaction expression for: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + CH_3CO_2H + PbO_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: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + 2 CH_3CO_2H + PbO_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 | 1 | -1 NaOCl | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 NaCl | 1 | 1 CH_3CO_2H | 2 | 2 PbO_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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) Pb(CH_3CO_2)_2 | 1 | -1 | -(Δ[Pb(CH3CO2)2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) CH_3CO_2H | 2 | 2 | 1/2 (Δ[CH3CO2H])/(Δt) PbO_2 | 1 | 1 | (Δ[PbO2])/(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[H2O])/(Δt) = -(Δ[NaOCl])/(Δt) = -(Δ[Pb(CH3CO2)2])/(Δt) = (Δ[NaCl])/(Δt) = 1/2 (Δ[CH3CO2H])/(Δt) = (Δ[PbO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + CH_3CO_2H + PbO_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: H_2O + NaOCl + Pb(CH_3CO_2)_2 ⟶ NaCl + 2 CH_3CO_2H + PbO_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 | 1 | -1 NaOCl | 1 | -1 Pb(CH_3CO_2)_2 | 1 | -1 NaCl | 1 | 1 CH_3CO_2H | 2 | 2 PbO_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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) Pb(CH_3CO_2)_2 | 1 | -1 | -(Δ[Pb(CH3CO2)2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) CH_3CO_2H | 2 | 2 | 1/2 (Δ[CH3CO2H])/(Δt) PbO_2 | 1 | 1 | (Δ[PbO2])/(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[H2O])/(Δt) = -(Δ[NaOCl])/(Δt) = -(Δ[Pb(CH3CO2)2])/(Δt) = (Δ[NaCl])/(Δt) = 1/2 (Δ[CH3CO2H])/(Δt) = (Δ[PbO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | sodium hypochlorite | lead(II) acetate | sodium chloride | acetic acid | lead dioxide formula | H_2O | NaOCl | Pb(CH_3CO_2)_2 | NaCl | CH_3CO_2H | PbO_2 Hill formula | H_2O | ClNaO | C_4H_6O_4Pb | ClNa | C_2H_4O_2 | O_2Pb name | water | sodium hypochlorite | lead(II) acetate | sodium chloride | acetic acid | lead dioxide IUPAC name | water | sodium hypochlorite | lead(2+) diacetate | sodium chloride | acetic acid |
| water | sodium hypochlorite | lead(II) acetate | sodium chloride | acetic acid | lead dioxide formula | H_2O | NaOCl | Pb(CH_3CO_2)_2 | NaCl | CH_3CO_2H | PbO_2 Hill formula | H_2O | ClNaO | C_4H_6O_4Pb | ClNa | C_2H_4O_2 | O_2Pb name | water | sodium hypochlorite | lead(II) acetate | sodium chloride | acetic acid | lead dioxide IUPAC name | water | sodium hypochlorite | lead(2+) diacetate | sodium chloride | acetic acid |

Random Queries

CAS perrhenic acid
molar mass of fmoc-phe-OH-2-13 C
density of 5-chloro-1-ethyl-2-methylimidazole
price of lead vs rhenium
ion class of thiocyanate anion vs nitrate anion
molar mass of butane vs cyclopropane
name of antimony pentachloride
net ionic charge of tin IV
element types of sodium hypochlorite vs titanium hydride
atomic diameter of period 3 elements