Input interpretation
N2O5H2O ⟶ HNO_3 nitric acid
Balanced equation
Balance the chemical equation algebraically: N2O5H2O ⟶ HNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 N2O5H2O ⟶ c_2 HNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for N, O and H: N: | 2 c_1 = c_2 O: | 6 c_1 = 3 c_2 H: | 2 c_1 = c_2 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | N2O5H2O ⟶ 2 HNO_3
Structures
N2O5H2O ⟶
Names
N2O5H2O ⟶ nitric acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: N2O5H2O ⟶ HNO_3 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: N2O5H2O ⟶ 2 HNO_3 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 N2O5H2O | 1 | -1 HNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression N2O5H2O | 1 | -1 | ([N2O5H2O])^(-1) HNO_3 | 2 | 2 | ([HNO3])^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 = ([N2O5H2O])^(-1) ([HNO3])^2 = ([HNO3])^2/([N2O5H2O])](../image_source/cc155f9a221de37b3727a76d84db4ecb.png)
Construct the equilibrium constant, K, expression for: N2O5H2O ⟶ HNO_3 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: N2O5H2O ⟶ 2 HNO_3 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 N2O5H2O | 1 | -1 HNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression N2O5H2O | 1 | -1 | ([N2O5H2O])^(-1) HNO_3 | 2 | 2 | ([HNO3])^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 = ([N2O5H2O])^(-1) ([HNO3])^2 = ([HNO3])^2/([N2O5H2O])
Rate of reaction
![Construct the rate of reaction expression for: N2O5H2O ⟶ HNO_3 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: N2O5H2O ⟶ 2 HNO_3 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 N2O5H2O | 1 | -1 HNO_3 | 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 N2O5H2O | 1 | -1 | -(Δ[N2O5H2O])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(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[N2O5H2O])/(Δt) = 1/2 (Δ[HNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/ab32f57260851c4e70ce8886883f41e0.png)
Construct the rate of reaction expression for: N2O5H2O ⟶ HNO_3 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: N2O5H2O ⟶ 2 HNO_3 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 N2O5H2O | 1 | -1 HNO_3 | 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 N2O5H2O | 1 | -1 | -(Δ[N2O5H2O])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(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[N2O5H2O])/(Δt) = 1/2 (Δ[HNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| N2O5H2O | nitric acid formula | N2O5H2O | HNO_3 Hill formula | H2N2O6 | HNO_3 name | | nitric acid
Substance properties
| N2O5H2O | nitric acid molar mass | 126.02 g/mol | 63.012 g/mol phase | | liquid (at STP) melting point | | -41.6 °C boiling point | | 83 °C density | | 1.5129 g/cm^3 solubility in water | | miscible dynamic viscosity | | 7.6×10^-4 Pa s (at 25 °C)
Units
