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H2O2 + AgO = H2O + O2 + Ag

Input interpretation

H_2O_2 hydrogen peroxide + AgO silver(II) oxide ⟶ H_2O water + O_2 oxygen + Ag silver
H_2O_2 hydrogen peroxide + AgO silver(II) oxide ⟶ H_2O water + O_2 oxygen + Ag silver

Balanced equation

Balance the chemical equation algebraically: H_2O_2 + AgO ⟶ H_2O + O_2 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 AgO ⟶ c_3 H_2O + c_4 O_2 + c_5 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Ag: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + c_2 = c_3 + 2 c_4 Ag: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 1 c_4 = c_2/2 + 1/2 c_5 = c_2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 1 and solve for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O_2 + AgO ⟶ H_2O + O_2 + Ag
Balance the chemical equation algebraically: H_2O_2 + AgO ⟶ H_2O + O_2 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 AgO ⟶ c_3 H_2O + c_4 O_2 + c_5 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Ag: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + c_2 = c_3 + 2 c_4 Ag: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 1 c_4 = c_2/2 + 1/2 c_5 = c_2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 1 and solve for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O_2 + AgO ⟶ H_2O + O_2 + Ag

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen peroxide + silver(II) oxide ⟶ water + oxygen + silver
hydrogen peroxide + silver(II) oxide ⟶ water + oxygen + silver

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O_2 + AgO ⟶ H_2O + O_2 + Ag 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_2 + AgO ⟶ H_2O + O_2 + Ag 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 | 1 | -1 AgO | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 Ag | 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_2 | 1 | -1 | ([H2O2])^(-1) AgO | 1 | -1 | ([AgO])^(-1) H_2O | 1 | 1 | [H2O] O_2 | 1 | 1 | [O2] Ag | 1 | 1 | [Ag] 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 = ([H2O2])^(-1) ([AgO])^(-1) [H2O] [O2] [Ag] = ([H2O] [O2] [Ag])/([H2O2] [AgO])
Construct the equilibrium constant, K, expression for: H_2O_2 + AgO ⟶ H_2O + O_2 + Ag 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_2 + AgO ⟶ H_2O + O_2 + Ag 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 | 1 | -1 AgO | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 Ag | 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_2 | 1 | -1 | ([H2O2])^(-1) AgO | 1 | -1 | ([AgO])^(-1) H_2O | 1 | 1 | [H2O] O_2 | 1 | 1 | [O2] Ag | 1 | 1 | [Ag] 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 = ([H2O2])^(-1) ([AgO])^(-1) [H2O] [O2] [Ag] = ([H2O] [O2] [Ag])/([H2O2] [AgO])

Rate of reaction

Construct the rate of reaction expression for: H_2O_2 + AgO ⟶ H_2O + O_2 + Ag 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_2 + AgO ⟶ H_2O + O_2 + Ag 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 | 1 | -1 AgO | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 Ag | 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_2 | 1 | -1 | -(Δ[H2O2])/(Δt) AgO | 1 | -1 | -(Δ[AgO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Ag | 1 | 1 | (Δ[Ag])/(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[H2O2])/(Δt) = -(Δ[AgO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O_2 + AgO ⟶ H_2O + O_2 + Ag 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_2 + AgO ⟶ H_2O + O_2 + Ag 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 | 1 | -1 AgO | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 Ag | 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_2 | 1 | -1 | -(Δ[H2O2])/(Δt) AgO | 1 | -1 | -(Δ[AgO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) Ag | 1 | 1 | (Δ[Ag])/(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[H2O2])/(Δt) = -(Δ[AgO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen peroxide | silver(II) oxide | water | oxygen | silver formula | H_2O_2 | AgO | H_2O | O_2 | Ag name | hydrogen peroxide | silver(II) oxide | water | oxygen | silver IUPAC name | hydrogen peroxide | oxosilver | water | molecular oxygen | silver
| hydrogen peroxide | silver(II) oxide | water | oxygen | silver formula | H_2O_2 | AgO | H_2O | O_2 | Ag name | hydrogen peroxide | silver(II) oxide | water | oxygen | silver IUPAC name | hydrogen peroxide | oxosilver | water | molecular oxygen | silver

Substance properties

| hydrogen peroxide | silver(II) oxide | water | oxygen | silver molar mass | 34.014 g/mol | 123.867 g/mol | 18.015 g/mol | 31.998 g/mol | 107.8682 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -0.43 °C | 100 °C | 0 °C | -218 °C | 960 °C boiling point | 150.2 °C | | 99.9839 °C | -183 °C | 2212 °C density | 1.44 g/cm^3 | 7.44 g/cm^3 | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 10.49 g/cm^3 solubility in water | miscible | | | | insoluble surface tension | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |
| hydrogen peroxide | silver(II) oxide | water | oxygen | silver molar mass | 34.014 g/mol | 123.867 g/mol | 18.015 g/mol | 31.998 g/mol | 107.8682 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -0.43 °C | 100 °C | 0 °C | -218 °C | 960 °C boiling point | 150.2 °C | | 99.9839 °C | -183 °C | 2212 °C density | 1.44 g/cm^3 | 7.44 g/cm^3 | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 10.49 g/cm^3 solubility in water | miscible | | | | insoluble surface tension | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |

Units

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