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HNO3 + K = H2O + NH3 + KNO3

Input interpretation

HNO_3 nitric acid + K potassium ⟶ H_2O water + NH_3 ammonia + KNO_3 potassium nitrate
HNO_3 nitric acid + K potassium ⟶ H_2O water + NH_3 ammonia + KNO_3 potassium nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + K ⟶ H_2O + NH_3 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 K ⟶ c_3 H_2O + c_4 NH_3 + c_5 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 + 3 c_4 N: | c_1 = c_4 + c_5 O: | 3 c_1 = c_3 + 3 c_5 K: | c_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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 9 c_2 = 8 c_3 = 3 c_4 = 1 c_5 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 HNO_3 + 8 K ⟶ 3 H_2O + NH_3 + 8 KNO_3
Balance the chemical equation algebraically: HNO_3 + K ⟶ H_2O + NH_3 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 K ⟶ c_3 H_2O + c_4 NH_3 + c_5 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 + 3 c_4 N: | c_1 = c_4 + c_5 O: | 3 c_1 = c_3 + 3 c_5 K: | c_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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 9 c_2 = 8 c_3 = 3 c_4 = 1 c_5 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 9 HNO_3 + 8 K ⟶ 3 H_2O + NH_3 + 8 KNO_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

nitric acid + potassium ⟶ water + ammonia + potassium nitrate
nitric acid + potassium ⟶ water + ammonia + potassium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + K ⟶ H_2O + NH_3 + 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: 9 HNO_3 + 8 K ⟶ 3 H_2O + NH_3 + 8 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 | 9 | -9 K | 8 | -8 H_2O | 3 | 3 NH_3 | 1 | 1 KNO_3 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 9 | -9 | ([HNO3])^(-9) K | 8 | -8 | ([K])^(-8) H_2O | 3 | 3 | ([H2O])^3 NH_3 | 1 | 1 | [NH3] KNO_3 | 8 | 8 | ([KNO3])^8 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])^(-9) ([K])^(-8) ([H2O])^3 [NH3] ([KNO3])^8 = (([H2O])^3 [NH3] ([KNO3])^8)/(([HNO3])^9 ([K])^8)
Construct the equilibrium constant, K, expression for: HNO_3 + K ⟶ H_2O + NH_3 + 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: 9 HNO_3 + 8 K ⟶ 3 H_2O + NH_3 + 8 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 | 9 | -9 K | 8 | -8 H_2O | 3 | 3 NH_3 | 1 | 1 KNO_3 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 9 | -9 | ([HNO3])^(-9) K | 8 | -8 | ([K])^(-8) H_2O | 3 | 3 | ([H2O])^3 NH_3 | 1 | 1 | [NH3] KNO_3 | 8 | 8 | ([KNO3])^8 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])^(-9) ([K])^(-8) ([H2O])^3 [NH3] ([KNO3])^8 = (([H2O])^3 [NH3] ([KNO3])^8)/(([HNO3])^9 ([K])^8)

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + K ⟶ H_2O + NH_3 + 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: 9 HNO_3 + 8 K ⟶ 3 H_2O + NH_3 + 8 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 | 9 | -9 K | 8 | -8 H_2O | 3 | 3 NH_3 | 1 | 1 KNO_3 | 8 | 8 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 | 9 | -9 | -1/9 (Δ[HNO3])/(Δt) K | 8 | -8 | -1/8 (Δ[K])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NH_3 | 1 | 1 | (Δ[NH3])/(Δt) KNO_3 | 8 | 8 | 1/8 (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 = -1/9 (Δ[HNO3])/(Δt) = -1/8 (Δ[K])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[NH3])/(Δt) = 1/8 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + K ⟶ H_2O + NH_3 + 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: 9 HNO_3 + 8 K ⟶ 3 H_2O + NH_3 + 8 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 | 9 | -9 K | 8 | -8 H_2O | 3 | 3 NH_3 | 1 | 1 KNO_3 | 8 | 8 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 | 9 | -9 | -1/9 (Δ[HNO3])/(Δt) K | 8 | -8 | -1/8 (Δ[K])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NH_3 | 1 | 1 | (Δ[NH3])/(Δt) KNO_3 | 8 | 8 | 1/8 (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 = -1/9 (Δ[HNO3])/(Δt) = -1/8 (Δ[K])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[NH3])/(Δt) = 1/8 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | potassium | water | ammonia | potassium nitrate formula | HNO_3 | K | H_2O | NH_3 | KNO_3 Hill formula | HNO_3 | K | H_2O | H_3N | KNO_3 name | nitric acid | potassium | water | ammonia | potassium nitrate
| nitric acid | potassium | water | ammonia | potassium nitrate formula | HNO_3 | K | H_2O | NH_3 | KNO_3 Hill formula | HNO_3 | K | H_2O | H_3N | KNO_3 name | nitric acid | potassium | water | ammonia | potassium nitrate

Substance properties

| nitric acid | potassium | water | ammonia | potassium nitrate molar mass | 63.012 g/mol | 39.0983 g/mol | 18.015 g/mol | 17.031 g/mol | 101.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | 64 °C | 0 °C | -77.73 °C | 334 °C boiling point | 83 °C | 760 °C | 99.9839 °C | -33.33 °C | density | 1.5129 g/cm^3 | 0.86 g/cm^3 | 1 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | solubility in water | miscible | reacts | | | soluble surface tension | | | 0.0728 N/m | 0.0234 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.009×10^-5 Pa s (at 25 °C) | odor | | | odorless | | odorless
| nitric acid | potassium | water | ammonia | potassium nitrate molar mass | 63.012 g/mol | 39.0983 g/mol | 18.015 g/mol | 17.031 g/mol | 101.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -41.6 °C | 64 °C | 0 °C | -77.73 °C | 334 °C boiling point | 83 °C | 760 °C | 99.9839 °C | -33.33 °C | density | 1.5129 g/cm^3 | 0.86 g/cm^3 | 1 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | solubility in water | miscible | reacts | | | soluble surface tension | | | 0.0728 N/m | 0.0234 N/m | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.009×10^-5 Pa s (at 25 °C) | odor | | | odorless | | odorless

Units

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