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H2SO4 + Pb = H2O + SO2 + Pb(HSO4)2

Input interpretation

H_2SO_4 (sulfuric acid) + Pb (lead) ⟶ H_2O (water) + SO_2 (sulfur dioxide) + Pb(HSO4)2
H_2SO_4 (sulfuric acid) + Pb (lead) ⟶ H_2O (water) + SO_2 (sulfur dioxide) + Pb(HSO4)2

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + Pb ⟶ H_2O + SO_2 + Pb(HSO4)2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Pb ⟶ c_3 H_2O + c_4 SO_2 + c_5 Pb(HSO4)2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Pb: H: | 2 c_1 = 2 c_3 + 2 c_5 O: | 4 c_1 = c_3 + 2 c_4 + 8 c_5 S: | c_1 = c_4 + 2 c_5 Pb: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + Pb ⟶ 2 H_2O + SO_2 + Pb(HSO4)2
Balance the chemical equation algebraically: H_2SO_4 + Pb ⟶ H_2O + SO_2 + Pb(HSO4)2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Pb ⟶ c_3 H_2O + c_4 SO_2 + c_5 Pb(HSO4)2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Pb: H: | 2 c_1 = 2 c_3 + 2 c_5 O: | 4 c_1 = c_3 + 2 c_4 + 8 c_5 S: | c_1 = c_4 + 2 c_5 Pb: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + Pb ⟶ 2 H_2O + SO_2 + Pb(HSO4)2

Structures

+ ⟶ + + Pb(HSO4)2
+ ⟶ + + Pb(HSO4)2

Names

sulfuric acid + lead ⟶ water + sulfur dioxide + Pb(HSO4)2
sulfuric acid + lead ⟶ water + sulfur dioxide + Pb(HSO4)2

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + Pb ⟶ H_2O + SO_2 + Pb(HSO4)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: 3 H_2SO_4 + Pb ⟶ 2 H_2O + SO_2 + Pb(HSO4)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_2SO_4 | 3 | -3 Pb | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(HSO4)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_2SO_4 | 3 | -3 | ([H2SO4])^(-3) Pb | 1 | -1 | ([Pb])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] Pb(HSO4)2 | 1 | 1 | [Pb(HSO4)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 = ([H2SO4])^(-3) ([Pb])^(-1) ([H2O])^2 [SO2] [Pb(HSO4)2] = (([H2O])^2 [SO2] [Pb(HSO4)2])/(([H2SO4])^3 [Pb])
Construct the equilibrium constant, K, expression for: H_2SO_4 + Pb ⟶ H_2O + SO_2 + Pb(HSO4)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: 3 H_2SO_4 + Pb ⟶ 2 H_2O + SO_2 + Pb(HSO4)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_2SO_4 | 3 | -3 Pb | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(HSO4)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_2SO_4 | 3 | -3 | ([H2SO4])^(-3) Pb | 1 | -1 | ([Pb])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] Pb(HSO4)2 | 1 | 1 | [Pb(HSO4)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 = ([H2SO4])^(-3) ([Pb])^(-1) ([H2O])^2 [SO2] [Pb(HSO4)2] = (([H2O])^2 [SO2] [Pb(HSO4)2])/(([H2SO4])^3 [Pb])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + Pb ⟶ H_2O + SO_2 + Pb(HSO4)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: 3 H_2SO_4 + Pb ⟶ 2 H_2O + SO_2 + Pb(HSO4)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_2SO_4 | 3 | -3 Pb | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(HSO4)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_2SO_4 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) Pb | 1 | -1 | -(Δ[Pb])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) Pb(HSO4)2 | 1 | 1 | (Δ[Pb(HSO4)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 = -1/3 (Δ[H2SO4])/(Δt) = -(Δ[Pb])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[Pb(HSO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + Pb ⟶ H_2O + SO_2 + Pb(HSO4)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: 3 H_2SO_4 + Pb ⟶ 2 H_2O + SO_2 + Pb(HSO4)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_2SO_4 | 3 | -3 Pb | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Pb(HSO4)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_2SO_4 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) Pb | 1 | -1 | -(Δ[Pb])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) Pb(HSO4)2 | 1 | 1 | (Δ[Pb(HSO4)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 = -1/3 (Δ[H2SO4])/(Δt) = -(Δ[Pb])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[Pb(HSO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | lead | water | sulfur dioxide | Pb(HSO4)2 formula | H_2SO_4 | Pb | H_2O | SO_2 | Pb(HSO4)2 Hill formula | H_2O_4S | Pb | H_2O | O_2S | H2O8PbS2 name | sulfuric acid | lead | water | sulfur dioxide |
| sulfuric acid | lead | water | sulfur dioxide | Pb(HSO4)2 formula | H_2SO_4 | Pb | H_2O | SO_2 | Pb(HSO4)2 Hill formula | H_2O_4S | Pb | H_2O | O_2S | H2O8PbS2 name | sulfuric acid | lead | water | sulfur dioxide |

Substance properties

| sulfuric acid | lead | water | sulfur dioxide | Pb(HSO4)2 molar mass | 98.07 g/mol | 207.2 g/mol | 18.015 g/mol | 64.06 g/mol | 401.3 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | 10.371 °C | 327.4 °C | 0 °C | -73 °C | boiling point | 279.6 °C | 1740 °C | 99.9839 °C | -10 °C | density | 1.8305 g/cm^3 | 11.34 g/cm^3 | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | solubility in water | very soluble | insoluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | 0.02859 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.00183 Pa s (at 38 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless | |
| sulfuric acid | lead | water | sulfur dioxide | Pb(HSO4)2 molar mass | 98.07 g/mol | 207.2 g/mol | 18.015 g/mol | 64.06 g/mol | 401.3 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | melting point | 10.371 °C | 327.4 °C | 0 °C | -73 °C | boiling point | 279.6 °C | 1740 °C | 99.9839 °C | -10 °C | density | 1.8305 g/cm^3 | 11.34 g/cm^3 | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | solubility in water | very soluble | insoluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | 0.02859 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.00183 Pa s (at 38 °C) | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless | |

Units

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