Input interpretation
![HNO_3 nitric acid ⟶ H_2O water + N_2O_5 dinitrogen pentoxide](../image_source/369ae4a0c8c6e511bba4d667752b56b4.png)
HNO_3 nitric acid ⟶ H_2O water + N_2O_5 dinitrogen pentoxide
Balanced equation
![Balance the chemical equation algebraically: HNO_3 ⟶ H_2O + N_2O_5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 ⟶ c_2 H_2O + c_3 N_2O_5 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N and O: H: | c_1 = 2 c_2 N: | c_1 = 2 c_3 O: | 3 c_1 = c_2 + 5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 ⟶ H_2O + N_2O_5](../image_source/9c06d467303ef131f949bfb52f43b3f2.png)
Balance the chemical equation algebraically: HNO_3 ⟶ H_2O + N_2O_5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 ⟶ c_2 H_2O + c_3 N_2O_5 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N and O: H: | c_1 = 2 c_2 N: | c_1 = 2 c_3 O: | 3 c_1 = c_2 + 5 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 ⟶ H_2O + N_2O_5
Structures
![⟶ +](../image_source/2db2b28a48489b173e378fb76e847fe2.png)
⟶ +
Names
![nitric acid ⟶ water + dinitrogen pentoxide](../image_source/4a48e81c72844add3e9a1c975a1e60f6.png)
nitric acid ⟶ water + dinitrogen pentoxide
Reaction thermodynamics
Gibbs free energy
![| nitric acid | water | dinitrogen pentoxide molecular free energy | -80.7 kJ/mol | -237.1 kJ/mol | 113.9 kJ/mol total free energy | -161.4 kJ/mol | -237.1 kJ/mol | 113.9 kJ/mol | G_initial = -161.4 kJ/mol | G_final = -123.2 kJ/mol | ΔG_rxn^0 | -123.2 kJ/mol - -161.4 kJ/mol = 38.2 kJ/mol (endergonic) | |](../image_source/999f47abf963185f84f3dcc696445433.png)
| nitric acid | water | dinitrogen pentoxide molecular free energy | -80.7 kJ/mol | -237.1 kJ/mol | 113.9 kJ/mol total free energy | -161.4 kJ/mol | -237.1 kJ/mol | 113.9 kJ/mol | G_initial = -161.4 kJ/mol | G_final = -123.2 kJ/mol | ΔG_rxn^0 | -123.2 kJ/mol - -161.4 kJ/mol = 38.2 kJ/mol (endergonic) | |
Entropy
![| nitric acid | water | dinitrogen pentoxide molecular entropy | 156 J/(mol K) | 69.91 J/(mol K) | 178 J/(mol K) total entropy | 312 J/(mol K) | 69.91 J/(mol K) | 178 J/(mol K) | S_initial = 312 J/(mol K) | S_final = 247.9 J/(mol K) | ΔS_rxn^0 | 247.9 J/(mol K) - 312 J/(mol K) = -64.09 J/(mol K) (exoentropic) | |](../image_source/8d57d742cff0dc6e0f82c9bbe4682b46.png)
| nitric acid | water | dinitrogen pentoxide molecular entropy | 156 J/(mol K) | 69.91 J/(mol K) | 178 J/(mol K) total entropy | 312 J/(mol K) | 69.91 J/(mol K) | 178 J/(mol K) | S_initial = 312 J/(mol K) | S_final = 247.9 J/(mol K) | ΔS_rxn^0 | 247.9 J/(mol K) - 312 J/(mol K) = -64.09 J/(mol K) (exoentropic) | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 | 2 | -2 H_2O | 1 | 1 N_2O_5 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) H_2O | 1 | 1 | [H2O] N_2O_5 | 1 | 1 | [N2O5] 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 = ([HNO3])^(-2) [H2O] [N2O5] = ([H2O] [N2O5])/([HNO3])^2](../image_source/abfe0a6b86d1737d9dc6c4e1f2e908d2.png)
Construct the equilibrium constant, K, expression for: HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 | 2 | -2 H_2O | 1 | 1 N_2O_5 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) H_2O | 1 | 1 | [H2O] N_2O_5 | 1 | 1 | [N2O5] 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 = ([HNO3])^(-2) [H2O] [N2O5] = ([H2O] [N2O5])/([HNO3])^2
Rate of reaction
![Construct the rate of reaction expression for: HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 | 2 | -2 H_2O | 1 | 1 N_2O_5 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) N_2O_5 | 1 | 1 | (Δ[N2O5])/(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[HNO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[N2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/1a8d3e0a737179511072aa96f1ff3129.png)
Construct the rate of reaction expression for: HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 ⟶ H_2O + N_2O_5 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 HNO_3 | 2 | -2 H_2O | 1 | 1 N_2O_5 | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) N_2O_5 | 1 | 1 | (Δ[N2O5])/(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[HNO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[N2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| nitric acid | water | dinitrogen pentoxide formula | HNO_3 | H_2O | N_2O_5 name | nitric acid | water | dinitrogen pentoxide IUPAC name | nitric acid | water | nitro nitrate](../image_source/8ccee0c4a10949726e96dcf4f072ef8d.png)
| nitric acid | water | dinitrogen pentoxide formula | HNO_3 | H_2O | N_2O_5 name | nitric acid | water | dinitrogen pentoxide IUPAC name | nitric acid | water | nitro nitrate
Substance properties
![| nitric acid | water | dinitrogen pentoxide molar mass | 63.012 g/mol | 18.015 g/mol | 108.01 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | -41.6 °C | 0 °C | 30 °C boiling point | 83 °C | 99.9839 °C | 47 °C density | 1.5129 g/cm^3 | 1 g/cm^3 | 2.05 g/cm^3 solubility in water | miscible | | surface tension | | 0.0728 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless |](../image_source/524bf75f3db225bf90997867f1ecd7b2.png)
| nitric acid | water | dinitrogen pentoxide molar mass | 63.012 g/mol | 18.015 g/mol | 108.01 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | -41.6 °C | 0 °C | 30 °C boiling point | 83 °C | 99.9839 °C | 47 °C density | 1.5129 g/cm^3 | 1 g/cm^3 | 2.05 g/cm^3 solubility in water | miscible | | surface tension | | 0.0728 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless |
Units