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H2O + AgNO3 = O2 + HNO3 + Ag

Input interpretation

H_2O water + AgNO_3 silver nitrate ⟶ O_2 oxygen + HNO_3 nitric acid + Ag silver
H_2O water + AgNO_3 silver nitrate ⟶ O_2 oxygen + HNO_3 nitric acid + Ag silver

Balanced equation

Balance the chemical equation algebraically: H_2O + AgNO_3 ⟶ O_2 + HNO_3 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 AgNO_3 ⟶ c_3 O_2 + c_4 HNO_3 + c_5 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ag and N: H: | 2 c_1 = c_4 O: | c_1 + 3 c_2 = 2 c_3 + 3 c_4 Ag: | c_2 = c_5 N: | 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 = 4 c_3 = 1 c_4 = 4 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 4 AgNO_3 ⟶ O_2 + 4 HNO_3 + 4 Ag
Balance the chemical equation algebraically: H_2O + AgNO_3 ⟶ O_2 + HNO_3 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 AgNO_3 ⟶ c_3 O_2 + c_4 HNO_3 + c_5 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ag and N: H: | 2 c_1 = c_4 O: | c_1 + 3 c_2 = 2 c_3 + 3 c_4 Ag: | c_2 = c_5 N: | 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 = 4 c_3 = 1 c_4 = 4 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 4 AgNO_3 ⟶ O_2 + 4 HNO_3 + 4 Ag

Structures

+ ⟶ + +
+ ⟶ + +

Names

water + silver nitrate ⟶ oxygen + nitric acid + silver
water + silver nitrate ⟶ oxygen + nitric acid + silver

Reaction thermodynamics

Entropy

| water | silver nitrate | oxygen | nitric acid | silver molecular entropy | 69.91 J/(mol K) | 140.9 J/(mol K) | 205 J/(mol K) | 156 J/(mol K) | 42.6 J/(mol K) total entropy | 139.8 J/(mol K) | 563.6 J/(mol K) | 205 J/(mol K) | 624 J/(mol K) | 170.4 J/(mol K) | S_initial = 703.4 J/(mol K) | | S_final = 999.4 J/(mol K) | | ΔS_rxn^0 | 999.4 J/(mol K) - 703.4 J/(mol K) = 296 J/(mol K) (endoentropic) | | | |
| water | silver nitrate | oxygen | nitric acid | silver molecular entropy | 69.91 J/(mol K) | 140.9 J/(mol K) | 205 J/(mol K) | 156 J/(mol K) | 42.6 J/(mol K) total entropy | 139.8 J/(mol K) | 563.6 J/(mol K) | 205 J/(mol K) | 624 J/(mol K) | 170.4 J/(mol K) | S_initial = 703.4 J/(mol K) | | S_final = 999.4 J/(mol K) | | ΔS_rxn^0 | 999.4 J/(mol K) - 703.4 J/(mol K) = 296 J/(mol K) (endoentropic) | | | |

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + AgNO_3 ⟶ O_2 + HNO_3 + 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 H_2O + 4 AgNO_3 ⟶ O_2 + 4 HNO_3 + 4 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 | -2 AgNO_3 | 4 | -4 O_2 | 1 | 1 HNO_3 | 4 | 4 Ag | 4 | 4 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) AgNO_3 | 4 | -4 | ([AgNO3])^(-4) O_2 | 1 | 1 | [O2] HNO_3 | 4 | 4 | ([HNO3])^4 Ag | 4 | 4 | ([Ag])^4 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) ([AgNO3])^(-4) [O2] ([HNO3])^4 ([Ag])^4 = ([O2] ([HNO3])^4 ([Ag])^4)/(([H2O])^2 ([AgNO3])^4)
Construct the equilibrium constant, K, expression for: H_2O + AgNO_3 ⟶ O_2 + HNO_3 + 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 H_2O + 4 AgNO_3 ⟶ O_2 + 4 HNO_3 + 4 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 | -2 AgNO_3 | 4 | -4 O_2 | 1 | 1 HNO_3 | 4 | 4 Ag | 4 | 4 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) AgNO_3 | 4 | -4 | ([AgNO3])^(-4) O_2 | 1 | 1 | [O2] HNO_3 | 4 | 4 | ([HNO3])^4 Ag | 4 | 4 | ([Ag])^4 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) ([AgNO3])^(-4) [O2] ([HNO3])^4 ([Ag])^4 = ([O2] ([HNO3])^4 ([Ag])^4)/(([H2O])^2 ([AgNO3])^4)

Rate of reaction

Construct the rate of reaction expression for: H_2O + AgNO_3 ⟶ O_2 + HNO_3 + 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 H_2O + 4 AgNO_3 ⟶ O_2 + 4 HNO_3 + 4 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 | -2 AgNO_3 | 4 | -4 O_2 | 1 | 1 HNO_3 | 4 | 4 Ag | 4 | 4 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) AgNO_3 | 4 | -4 | -1/4 (Δ[AgNO3])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) HNO_3 | 4 | 4 | 1/4 (Δ[HNO3])/(Δt) Ag | 4 | 4 | 1/4 (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[H2O])/(Δt) = -1/4 (Δ[AgNO3])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[HNO3])/(Δt) = 1/4 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + AgNO_3 ⟶ O_2 + HNO_3 + 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 H_2O + 4 AgNO_3 ⟶ O_2 + 4 HNO_3 + 4 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 | -2 AgNO_3 | 4 | -4 O_2 | 1 | 1 HNO_3 | 4 | 4 Ag | 4 | 4 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) AgNO_3 | 4 | -4 | -1/4 (Δ[AgNO3])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) HNO_3 | 4 | 4 | 1/4 (Δ[HNO3])/(Δt) Ag | 4 | 4 | 1/4 (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[H2O])/(Δt) = -1/4 (Δ[AgNO3])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[HNO3])/(Δt) = 1/4 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | silver nitrate | oxygen | nitric acid | silver formula | H_2O | AgNO_3 | O_2 | HNO_3 | Ag name | water | silver nitrate | oxygen | nitric acid | silver IUPAC name | water | silver nitrate | molecular oxygen | nitric acid | silver
| water | silver nitrate | oxygen | nitric acid | silver formula | H_2O | AgNO_3 | O_2 | HNO_3 | Ag name | water | silver nitrate | oxygen | nitric acid | silver IUPAC name | water | silver nitrate | molecular oxygen | nitric acid | silver

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