HNO3 + K2O = H2O + KNO3

HNO_3 nitric acid + K_2O potassium oxide ⟶ H_2O water + KNO_3 potassium nitrate

Balance the chemical equation algebraically: HNO_3 + K_2O ⟶ H_2O + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 K_2O ⟶ c_3 H_2O + c_4 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and K: H: | c_1 = 2 c_3 N: | c_1 = c_4 O: | 3 c_1 + c_2 = c_3 + 3 c_4 K: | 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 + K_2O ⟶ H_2O + 2 KNO_3

+ ⟶ +

nitric acid + potassium oxide ⟶ water + potassium nitrate

Construct the equilibrium constant, K, expression for: HNO_3 + K_2O ⟶ H_2O + KNO_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: 2 HNO_3 + K_2O ⟶ H_2O + 2 KNO_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 HNO_3 | 2 | -2 K_2O | 1 | -1 H_2O | 1 | 1 KNO_3 | 2 | 2 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) K_2O | 1 | -1 | ([K2O])^(-1) H_2O | 1 | 1 | [H2O] KNO_3 | 2 | 2 | ([KNO3])^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 = ([HNO3])^(-2) ([K2O])^(-1) [H2O] ([KNO3])^2 = ([H2O] ([KNO3])^2)/(([HNO3])^2 [K2O])

Construct the rate of reaction expression for: HNO_3 + K_2O ⟶ H_2O + KNO_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: 2 HNO_3 + K_2O ⟶ H_2O + 2 KNO_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 HNO_3 | 2 | -2 K_2O | 1 | -1 H_2O | 1 | 1 KNO_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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) K_2O | 1 | -1 | -(Δ[K2O])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(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[K2O])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| nitric acid | potassium oxide | water | potassium nitrate formula | HNO_3 | K_2O | H_2O | KNO_3 name | nitric acid | potassium oxide | water | potassium nitrate IUPAC name | nitric acid | dipotassium oxygen(2-) | water | potassium nitrate

| nitric acid | potassium oxide | water | potassium nitrate molar mass | 63.012 g/mol | 94.196 g/mol | 18.015 g/mol | 101.1 g/mol phase | liquid (at STP) | | liquid (at STP) | solid (at STP) melting point | -41.6 °C | | 0 °C | 334 °C boiling point | 83 °C | | 99.9839 °C | density | 1.5129 g/cm^3 | | 1 g/cm^3 | solubility in water | miscible | | | soluble 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 | odorless