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H2O + HNO3 + P = NO + H3PO3

Input interpretation

H_2O water + HNO_3 nitric acid + P red phosphorus ⟶ NO nitric oxide + HP(O)(OH)_2 phosphorous acid
H_2O water + HNO_3 nitric acid + P red phosphorus ⟶ NO nitric oxide + HP(O)(OH)_2 phosphorous acid

Balanced equation

Balance the chemical equation algebraically: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 P ⟶ c_4 NO + c_5 HP(O)(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and P: H: | 2 c_1 + c_2 = 3 c_5 O: | c_1 + 3 c_2 = c_4 + 3 c_5 N: | c_2 = c_4 P: | c_3 = 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_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_2
Balance the chemical equation algebraically: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 P ⟶ c_4 NO + c_5 HP(O)(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and P: H: | 2 c_1 + c_2 = 3 c_5 O: | c_1 + 3 c_2 = c_4 + 3 c_5 N: | c_2 = c_4 P: | c_3 = 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_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_2

Structures

+ + ⟶ +
+ + ⟶ +

Names

water + nitric acid + red phosphorus ⟶ nitric oxide + phosphorous acid
water + nitric acid + red phosphorus ⟶ nitric oxide + phosphorous acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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 H_2O | 1 | -1 HNO_3 | 1 | -1 P | 1 | -1 NO | 1 | 1 HP(O)(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) HNO_3 | 1 | -1 | ([HNO3])^(-1) P | 1 | -1 | ([P])^(-1) NO | 1 | 1 | [NO] HP(O)(OH)_2 | 1 | 1 | [HP(O)(OH)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 = ([H2O])^(-1) ([HNO3])^(-1) ([P])^(-1) [NO] [HP(O)(OH)2] = ([NO] [HP(O)(OH)2])/([H2O] [HNO3] [P])
Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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 H_2O | 1 | -1 HNO_3 | 1 | -1 P | 1 | -1 NO | 1 | 1 HP(O)(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) HNO_3 | 1 | -1 | ([HNO3])^(-1) P | 1 | -1 | ([P])^(-1) NO | 1 | 1 | [NO] HP(O)(OH)_2 | 1 | 1 | [HP(O)(OH)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 = ([H2O])^(-1) ([HNO3])^(-1) ([P])^(-1) [NO] [HP(O)(OH)2] = ([NO] [HP(O)(OH)2])/([H2O] [HNO3] [P])

Rate of reaction

Construct the rate of reaction expression for: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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 H_2O | 1 | -1 HNO_3 | 1 | -1 P | 1 | -1 NO | 1 | 1 HP(O)(OH)_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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) P | 1 | -1 | -(Δ[P])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) HP(O)(OH)_2 | 1 | 1 | (Δ[HP(O)(OH)2])/(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[H2O])/(Δt) = -(Δ[HNO3])/(Δt) = -(Δ[P])/(Δt) = (Δ[NO])/(Δt) = (Δ[HP(O)(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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: H_2O + HNO_3 + P ⟶ NO + HP(O)(OH)_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 H_2O | 1 | -1 HNO_3 | 1 | -1 P | 1 | -1 NO | 1 | 1 HP(O)(OH)_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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) P | 1 | -1 | -(Δ[P])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) HP(O)(OH)_2 | 1 | 1 | (Δ[HP(O)(OH)2])/(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[H2O])/(Δt) = -(Δ[HNO3])/(Δt) = -(Δ[P])/(Δt) = (Δ[NO])/(Δt) = (Δ[HP(O)(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | nitric acid | red phosphorus | nitric oxide | phosphorous acid formula | H_2O | HNO_3 | P | NO | HP(O)(OH)_2 Hill formula | H_2O | HNO_3 | P | NO | H_3O_3P name | water | nitric acid | red phosphorus | nitric oxide | phosphorous acid IUPAC name | water | nitric acid | phosphorus | nitric oxide | phosphorous acid
| water | nitric acid | red phosphorus | nitric oxide | phosphorous acid formula | H_2O | HNO_3 | P | NO | HP(O)(OH)_2 Hill formula | H_2O | HNO_3 | P | NO | H_3O_3P name | water | nitric acid | red phosphorus | nitric oxide | phosphorous acid IUPAC name | water | nitric acid | phosphorus | nitric oxide | phosphorous acid

Substance properties

| water | nitric acid | red phosphorus | nitric oxide | phosphorous acid molar mass | 18.015 g/mol | 63.012 g/mol | 30.973761998 g/mol | 30.006 g/mol | 81.995 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | -41.6 °C | 579.2 °C | -163.6 °C | 74 °C boiling point | 99.9839 °C | 83 °C | | -151.7 °C | density | 1 g/cm^3 | 1.5129 g/cm^3 | 2.16 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 1.597 g/cm^3 solubility in water | | miscible | insoluble | | surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 20.2 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | odorless | | | |
| water | nitric acid | red phosphorus | nitric oxide | phosphorous acid molar mass | 18.015 g/mol | 63.012 g/mol | 30.973761998 g/mol | 30.006 g/mol | 81.995 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | -41.6 °C | 579.2 °C | -163.6 °C | 74 °C boiling point | 99.9839 °C | 83 °C | | -151.7 °C | density | 1 g/cm^3 | 1.5129 g/cm^3 | 2.16 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 1.597 g/cm^3 solubility in water | | miscible | insoluble | | surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 20.2 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | odorless | | | |

Units

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