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NH3 + O3 = H2O + O2 + HNO2

Input interpretation

NH_3 ammonia + O_3 ozone ⟶ H_2O water + O_2 oxygen + HNO_2 nitrous acid
NH_3 ammonia + O_3 ozone ⟶ H_2O water + O_2 oxygen + HNO_2 nitrous acid

Balanced equation

Balance the chemical equation algebraically: NH_3 + O_3 ⟶ H_2O + O_2 + HNO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 O_3 ⟶ c_3 H_2O + c_4 O_2 + c_5 HNO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N and O: H: | 3 c_1 = 2 c_3 + c_5 N: | c_1 = c_5 O: | 3 c_2 = c_3 + 2 c_4 + 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 = (3 c_2)/2 - 3/2 c_5 = 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 3 and solve for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NH_3 + 3 O_3 ⟶ H_2O + 3 O_2 + HNO_2
Balance the chemical equation algebraically: NH_3 + O_3 ⟶ H_2O + O_2 + HNO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 O_3 ⟶ c_3 H_2O + c_4 O_2 + c_5 HNO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N and O: H: | 3 c_1 = 2 c_3 + c_5 N: | c_1 = c_5 O: | 3 c_2 = c_3 + 2 c_4 + 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 = (3 c_2)/2 - 3/2 c_5 = 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 3 and solve for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NH_3 + 3 O_3 ⟶ H_2O + 3 O_2 + HNO_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

ammonia + ozone ⟶ water + oxygen + nitrous acid
ammonia + ozone ⟶ water + oxygen + nitrous acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: NH_3 + O_3 ⟶ H_2O + O_2 + HNO_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: NH_3 + 3 O_3 ⟶ H_2O + 3 O_2 + HNO_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 NH_3 | 1 | -1 O_3 | 3 | -3 H_2O | 1 | 1 O_2 | 3 | 3 HNO_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 1 | -1 | ([NH3])^(-1) O_3 | 3 | -3 | ([O3])^(-3) H_2O | 1 | 1 | [H2O] O_2 | 3 | 3 | ([O2])^3 HNO_2 | 1 | 1 | [HNO2] 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 = ([NH3])^(-1) ([O3])^(-3) [H2O] ([O2])^3 [HNO2] = ([H2O] ([O2])^3 [HNO2])/([NH3] ([O3])^3)
Construct the equilibrium constant, K, expression for: NH_3 + O_3 ⟶ H_2O + O_2 + HNO_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: NH_3 + 3 O_3 ⟶ H_2O + 3 O_2 + HNO_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 NH_3 | 1 | -1 O_3 | 3 | -3 H_2O | 1 | 1 O_2 | 3 | 3 HNO_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 1 | -1 | ([NH3])^(-1) O_3 | 3 | -3 | ([O3])^(-3) H_2O | 1 | 1 | [H2O] O_2 | 3 | 3 | ([O2])^3 HNO_2 | 1 | 1 | [HNO2] 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 = ([NH3])^(-1) ([O3])^(-3) [H2O] ([O2])^3 [HNO2] = ([H2O] ([O2])^3 [HNO2])/([NH3] ([O3])^3)

Rate of reaction

Construct the rate of reaction expression for: NH_3 + O_3 ⟶ H_2O + O_2 + HNO_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: NH_3 + 3 O_3 ⟶ H_2O + 3 O_2 + HNO_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 NH_3 | 1 | -1 O_3 | 3 | -3 H_2O | 1 | 1 O_2 | 3 | 3 HNO_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 NH_3 | 1 | -1 | -(Δ[NH3])/(Δt) O_3 | 3 | -3 | -1/3 (Δ[O3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) HNO_2 | 1 | 1 | (Δ[HNO2])/(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[NH3])/(Δt) = -1/3 (Δ[O3])/(Δt) = (Δ[H2O])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[HNO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NH_3 + O_3 ⟶ H_2O + O_2 + HNO_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: NH_3 + 3 O_3 ⟶ H_2O + 3 O_2 + HNO_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 NH_3 | 1 | -1 O_3 | 3 | -3 H_2O | 1 | 1 O_2 | 3 | 3 HNO_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 NH_3 | 1 | -1 | -(Δ[NH3])/(Δt) O_3 | 3 | -3 | -1/3 (Δ[O3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) HNO_2 | 1 | 1 | (Δ[HNO2])/(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[NH3])/(Δt) = -1/3 (Δ[O3])/(Δt) = (Δ[H2O])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[HNO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| ammonia | ozone | water | oxygen | nitrous acid formula | NH_3 | O_3 | H_2O | O_2 | HNO_2 Hill formula | H_3N | O_3 | H_2O | O_2 | HNO_2 name | ammonia | ozone | water | oxygen | nitrous acid IUPAC name | ammonia | ozone | water | molecular oxygen | nitrous acid
| ammonia | ozone | water | oxygen | nitrous acid formula | NH_3 | O_3 | H_2O | O_2 | HNO_2 Hill formula | H_3N | O_3 | H_2O | O_2 | HNO_2 name | ammonia | ozone | water | oxygen | nitrous acid IUPAC name | ammonia | ozone | water | molecular oxygen | nitrous acid

Substance properties

| ammonia | ozone | water | oxygen | nitrous acid molar mass | 17.031 g/mol | 47.997 g/mol | 18.015 g/mol | 31.998 g/mol | 47.013 g/mol phase | gas (at STP) | gas (at STP) | liquid (at STP) | gas (at STP) | melting point | -77.73 °C | -192.2 °C | 0 °C | -218 °C | boiling point | -33.33 °C | -111.9 °C | 99.9839 °C | -183 °C | density | 6.96×10^-4 g/cm^3 (at 25 °C) | 0.001962 g/cm^3 (at 25 °C) | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | surface tension | 0.0234 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 1.009×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |
| ammonia | ozone | water | oxygen | nitrous acid molar mass | 17.031 g/mol | 47.997 g/mol | 18.015 g/mol | 31.998 g/mol | 47.013 g/mol phase | gas (at STP) | gas (at STP) | liquid (at STP) | gas (at STP) | melting point | -77.73 °C | -192.2 °C | 0 °C | -218 °C | boiling point | -33.33 °C | -111.9 °C | 99.9839 °C | -183 °C | density | 6.96×10^-4 g/cm^3 (at 25 °C) | 0.001962 g/cm^3 (at 25 °C) | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | surface tension | 0.0234 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 1.009×10^-5 Pa s (at 25 °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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