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H2 + HNO3 + P = NO + H3PO4

Input interpretation

H_2 hydrogen + HNO_3 nitric acid + P red phosphorus ⟶ NO nitric oxide + H_3PO_4 phosphoric acid
H_2 hydrogen + HNO_3 nitric acid + P red phosphorus ⟶ NO nitric oxide + H_3PO_4 phosphoric acid

Balanced equation

Balance the chemical equation algebraically: H_2 + HNO_3 + P ⟶ NO + H_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 HNO_3 + c_3 P ⟶ c_4 NO + c_5 H_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and P: H: | 2 c_1 + c_2 = 3 c_5 N: | c_2 = c_4 O: | 3 c_2 = c_4 + 4 c_5 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 = 4 c_3 = 2 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + 4 HNO_3 + 2 P ⟶ 4 NO + 2 H_3PO_4
Balance the chemical equation algebraically: H_2 + HNO_3 + P ⟶ NO + H_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 HNO_3 + c_3 P ⟶ c_4 NO + c_5 H_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and P: H: | 2 c_1 + c_2 = 3 c_5 N: | c_2 = c_4 O: | 3 c_2 = c_4 + 4 c_5 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 = 4 c_3 = 2 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + 4 HNO_3 + 2 P ⟶ 4 NO + 2 H_3PO_4

Structures

+ + ⟶ +
+ + ⟶ +

Names

hydrogen + nitric acid + red phosphorus ⟶ nitric oxide + phosphoric acid
hydrogen + nitric acid + red phosphorus ⟶ nitric oxide + phosphoric acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2 + HNO_3 + P ⟶ NO + H_3PO_4 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_2 + 4 HNO_3 + 2 P ⟶ 4 NO + 2 H_3PO_4 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_2 | 1 | -1 HNO_3 | 4 | -4 P | 2 | -2 NO | 4 | 4 H_3PO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2 | 1 | -1 | ([H2])^(-1) HNO_3 | 4 | -4 | ([HNO3])^(-4) P | 2 | -2 | ([P])^(-2) NO | 4 | 4 | ([NO])^4 H_3PO_4 | 2 | 2 | ([H3PO4])^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 = ([H2])^(-1) ([HNO3])^(-4) ([P])^(-2) ([NO])^4 ([H3PO4])^2 = (([NO])^4 ([H3PO4])^2)/([H2] ([HNO3])^4 ([P])^2)
Construct the equilibrium constant, K, expression for: H_2 + HNO_3 + P ⟶ NO + H_3PO_4 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_2 + 4 HNO_3 + 2 P ⟶ 4 NO + 2 H_3PO_4 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_2 | 1 | -1 HNO_3 | 4 | -4 P | 2 | -2 NO | 4 | 4 H_3PO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2 | 1 | -1 | ([H2])^(-1) HNO_3 | 4 | -4 | ([HNO3])^(-4) P | 2 | -2 | ([P])^(-2) NO | 4 | 4 | ([NO])^4 H_3PO_4 | 2 | 2 | ([H3PO4])^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 = ([H2])^(-1) ([HNO3])^(-4) ([P])^(-2) ([NO])^4 ([H3PO4])^2 = (([NO])^4 ([H3PO4])^2)/([H2] ([HNO3])^4 ([P])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2 + HNO_3 + P ⟶ NO + H_3PO_4 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_2 + 4 HNO_3 + 2 P ⟶ 4 NO + 2 H_3PO_4 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_2 | 1 | -1 HNO_3 | 4 | -4 P | 2 | -2 NO | 4 | 4 H_3PO_4 | 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 H_2 | 1 | -1 | -(Δ[H2])/(Δt) HNO_3 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) P | 2 | -2 | -1/2 (Δ[P])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(Δt) H_3PO_4 | 2 | 2 | 1/2 (Δ[H3PO4])/(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[H2])/(Δt) = -1/4 (Δ[HNO3])/(Δt) = -1/2 (Δ[P])/(Δt) = 1/4 (Δ[NO])/(Δt) = 1/2 (Δ[H3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2 + HNO_3 + P ⟶ NO + H_3PO_4 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_2 + 4 HNO_3 + 2 P ⟶ 4 NO + 2 H_3PO_4 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_2 | 1 | -1 HNO_3 | 4 | -4 P | 2 | -2 NO | 4 | 4 H_3PO_4 | 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 H_2 | 1 | -1 | -(Δ[H2])/(Δt) HNO_3 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) P | 2 | -2 | -1/2 (Δ[P])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(Δt) H_3PO_4 | 2 | 2 | 1/2 (Δ[H3PO4])/(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[H2])/(Δt) = -1/4 (Δ[HNO3])/(Δt) = -1/2 (Δ[P])/(Δt) = 1/4 (Δ[NO])/(Δt) = 1/2 (Δ[H3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen | nitric acid | red phosphorus | nitric oxide | phosphoric acid formula | H_2 | HNO_3 | P | NO | H_3PO_4 Hill formula | H_2 | HNO_3 | P | NO | H_3O_4P name | hydrogen | nitric acid | red phosphorus | nitric oxide | phosphoric acid IUPAC name | molecular hydrogen | nitric acid | phosphorus | nitric oxide | phosphoric acid
| hydrogen | nitric acid | red phosphorus | nitric oxide | phosphoric acid formula | H_2 | HNO_3 | P | NO | H_3PO_4 Hill formula | H_2 | HNO_3 | P | NO | H_3O_4P name | hydrogen | nitric acid | red phosphorus | nitric oxide | phosphoric acid IUPAC name | molecular hydrogen | nitric acid | phosphorus | nitric oxide | phosphoric acid

Substance properties

| hydrogen | nitric acid | red phosphorus | nitric oxide | phosphoric acid molar mass | 2.016 g/mol | 63.012 g/mol | 30.973761998 g/mol | 30.006 g/mol | 97.994 g/mol phase | gas (at STP) | liquid (at STP) | solid (at STP) | gas (at STP) | liquid (at STP) melting point | -259.2 °C | -41.6 °C | 579.2 °C | -163.6 °C | 42.4 °C boiling point | -252.8 °C | 83 °C | | -151.7 °C | 158 °C density | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 2.16 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 1.685 g/cm^3 solubility in water | | miscible | insoluble | | very soluble dynamic viscosity | 8.9×10^-6 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 | | | | odorless
| hydrogen | nitric acid | red phosphorus | nitric oxide | phosphoric acid molar mass | 2.016 g/mol | 63.012 g/mol | 30.973761998 g/mol | 30.006 g/mol | 97.994 g/mol phase | gas (at STP) | liquid (at STP) | solid (at STP) | gas (at STP) | liquid (at STP) melting point | -259.2 °C | -41.6 °C | 579.2 °C | -163.6 °C | 42.4 °C boiling point | -252.8 °C | 83 °C | | -151.7 °C | 158 °C density | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 2.16 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 1.685 g/cm^3 solubility in water | | miscible | insoluble | | very soluble dynamic viscosity | 8.9×10^-6 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 | | | | odorless

Units

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