Input interpretation
![Ag(NO3)3 ⟶ O_2 oxygen + NO_2 nitrogen dioxide + Ag silver](../image_source/5f4c46df8a6c4f06443ed027f4474058.png)
Ag(NO3)3 ⟶ O_2 oxygen + NO_2 nitrogen dioxide + Ag silver
Balanced equation
![Balance the chemical equation algebraically: Ag(NO3)3 ⟶ O_2 + NO_2 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag(NO3)3 ⟶ c_2 O_2 + c_3 NO_2 + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N and O: Ag: | c_1 = c_4 N: | 3 c_1 = c_3 O: | 9 c_1 = 2 c_2 + 2 c_3 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 = 3/2 c_3 = 3 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 6 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Ag(NO3)3 ⟶ 3 O_2 + 6 NO_2 + 2 Ag](../image_source/3ef03caee93b9f9e95b6de351b73835d.png)
Balance the chemical equation algebraically: Ag(NO3)3 ⟶ O_2 + NO_2 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag(NO3)3 ⟶ c_2 O_2 + c_3 NO_2 + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N and O: Ag: | c_1 = c_4 N: | 3 c_1 = c_3 O: | 9 c_1 = 2 c_2 + 2 c_3 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 = 3/2 c_3 = 3 c_4 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 6 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Ag(NO3)3 ⟶ 3 O_2 + 6 NO_2 + 2 Ag
Structures
![Ag(NO3)3 ⟶ + +](../image_source/69be9996e9c538ff2675daf53bfc3841.png)
Ag(NO3)3 ⟶ + +
Names
![Ag(NO3)3 ⟶ oxygen + nitrogen dioxide + silver](../image_source/f9c2dd1427e58939d8d390f68d96a573.png)
Ag(NO3)3 ⟶ oxygen + nitrogen dioxide + silver
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Ag(NO3)3 ⟶ O_2 + NO_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: 2 Ag(NO3)3 ⟶ 3 O_2 + 6 NO_2 + 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 Ag(NO3)3 | 2 | -2 O_2 | 3 | 3 NO_2 | 6 | 6 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag(NO3)3 | 2 | -2 | ([Ag(NO3)3])^(-2) O_2 | 3 | 3 | ([O2])^3 NO_2 | 6 | 6 | ([NO2])^6 Ag | 2 | 2 | ([Ag])^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 = ([Ag(NO3)3])^(-2) ([O2])^3 ([NO2])^6 ([Ag])^2 = (([O2])^3 ([NO2])^6 ([Ag])^2)/([Ag(NO3)3])^2](../image_source/64bd119108e873acf0d73f14ba843e76.png)
Construct the equilibrium constant, K, expression for: Ag(NO3)3 ⟶ O_2 + NO_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: 2 Ag(NO3)3 ⟶ 3 O_2 + 6 NO_2 + 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 Ag(NO3)3 | 2 | -2 O_2 | 3 | 3 NO_2 | 6 | 6 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag(NO3)3 | 2 | -2 | ([Ag(NO3)3])^(-2) O_2 | 3 | 3 | ([O2])^3 NO_2 | 6 | 6 | ([NO2])^6 Ag | 2 | 2 | ([Ag])^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 = ([Ag(NO3)3])^(-2) ([O2])^3 ([NO2])^6 ([Ag])^2 = (([O2])^3 ([NO2])^6 ([Ag])^2)/([Ag(NO3)3])^2
Rate of reaction
![Construct the rate of reaction expression for: Ag(NO3)3 ⟶ O_2 + NO_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: 2 Ag(NO3)3 ⟶ 3 O_2 + 6 NO_2 + 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 Ag(NO3)3 | 2 | -2 O_2 | 3 | 3 NO_2 | 6 | 6 Ag | 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 Ag(NO3)3 | 2 | -2 | -1/2 (Δ[Ag(NO3)3])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) NO_2 | 6 | 6 | 1/6 (Δ[NO2])/(Δt) Ag | 2 | 2 | 1/2 (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 = -1/2 (Δ[Ag(NO3)3])/(Δt) = 1/3 (Δ[O2])/(Δt) = 1/6 (Δ[NO2])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/16d465c5c2ae96b96d43ea6967212302.png)
Construct the rate of reaction expression for: Ag(NO3)3 ⟶ O_2 + NO_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: 2 Ag(NO3)3 ⟶ 3 O_2 + 6 NO_2 + 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 Ag(NO3)3 | 2 | -2 O_2 | 3 | 3 NO_2 | 6 | 6 Ag | 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 Ag(NO3)3 | 2 | -2 | -1/2 (Δ[Ag(NO3)3])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) NO_2 | 6 | 6 | 1/6 (Δ[NO2])/(Δt) Ag | 2 | 2 | 1/2 (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 = -1/2 (Δ[Ag(NO3)3])/(Δt) = 1/3 (Δ[O2])/(Δt) = 1/6 (Δ[NO2])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| Ag(NO3)3 | oxygen | nitrogen dioxide | silver formula | Ag(NO3)3 | O_2 | NO_2 | Ag Hill formula | AgN3O9 | O_2 | NO_2 | Ag name | | oxygen | nitrogen dioxide | silver IUPAC name | | molecular oxygen | Nitrogen dioxide | silver](../image_source/a3f912be0df443a977a4d671207852a2.png)
| Ag(NO3)3 | oxygen | nitrogen dioxide | silver formula | Ag(NO3)3 | O_2 | NO_2 | Ag Hill formula | AgN3O9 | O_2 | NO_2 | Ag name | | oxygen | nitrogen dioxide | silver IUPAC name | | molecular oxygen | Nitrogen dioxide | silver
Substance properties
![| Ag(NO3)3 | oxygen | nitrogen dioxide | silver molar mass | 293.88 g/mol | 31.998 g/mol | 46.005 g/mol | 107.8682 g/mol phase | | gas (at STP) | gas (at STP) | solid (at STP) melting point | | -218 °C | -11 °C | 960 °C boiling point | | -183 °C | 21 °C | 2212 °C density | | 0.001429 g/cm^3 (at 0 °C) | 0.00188 g/cm^3 (at 25 °C) | 10.49 g/cm^3 solubility in water | | | reacts | insoluble surface tension | | 0.01347 N/m | | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) | odor | | odorless | |](../image_source/4fea09bc59a94d20bf48706f371af59c.png)
| Ag(NO3)3 | oxygen | nitrogen dioxide | silver molar mass | 293.88 g/mol | 31.998 g/mol | 46.005 g/mol | 107.8682 g/mol phase | | gas (at STP) | gas (at STP) | solid (at STP) melting point | | -218 °C | -11 °C | 960 °C boiling point | | -183 °C | 21 °C | 2212 °C density | | 0.001429 g/cm^3 (at 0 °C) | 0.00188 g/cm^3 (at 25 °C) | 10.49 g/cm^3 solubility in water | | | reacts | insoluble surface tension | | 0.01347 N/m | | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) | odor | | odorless | |
Units