Input interpretation
![H_3PO_4 phosphoric acid ⟶ H_2O water + HPO_3 metaphosphoric acid](../image_source/c041689c4d8a896a113f4c5c962b220a.png)
H_3PO_4 phosphoric acid ⟶ H_2O water + HPO_3 metaphosphoric acid
Balanced equation
![Balance the chemical equation algebraically: H_3PO_4 ⟶ H_2O + HPO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_3PO_4 ⟶ c_2 H_2O + c_3 HPO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and P: H: | 3 c_1 = 2 c_2 + c_3 O: | 4 c_1 = c_2 + 3 c_3 P: | c_1 = c_3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_3PO_4 ⟶ H_2O + HPO_3](../image_source/7923c42ad3443a59528ca5eb3585a6e0.png)
Balance the chemical equation algebraically: H_3PO_4 ⟶ H_2O + HPO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_3PO_4 ⟶ c_2 H_2O + c_3 HPO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and P: H: | 3 c_1 = 2 c_2 + c_3 O: | 4 c_1 = c_2 + 3 c_3 P: | c_1 = c_3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_3PO_4 ⟶ H_2O + HPO_3
Structures
![⟶ +](../image_source/63daa17279f62440e68284e06b181b36.png)
⟶ +
Names
![phosphoric acid ⟶ water + metaphosphoric acid](../image_source/0ab3d0961ed0af504a9081ec9ddac252.png)
phosphoric acid ⟶ water + metaphosphoric acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_3PO_4 ⟶ H_2O + HPO_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: H_3PO_4 ⟶ H_2O + HPO_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 H_3PO_4 | 1 | -1 H_2O | 1 | 1 HPO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_3PO_4 | 1 | -1 | ([H3PO4])^(-1) H_2O | 1 | 1 | [H2O] HPO_3 | 1 | 1 | [HPO3] 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 = ([H3PO4])^(-1) [H2O] [HPO3] = ([H2O] [HPO3])/([H3PO4])](../image_source/b41a91be2fc5992286e09c6bbcefb831.png)
Construct the equilibrium constant, K, expression for: H_3PO_4 ⟶ H_2O + HPO_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: H_3PO_4 ⟶ H_2O + HPO_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 H_3PO_4 | 1 | -1 H_2O | 1 | 1 HPO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_3PO_4 | 1 | -1 | ([H3PO4])^(-1) H_2O | 1 | 1 | [H2O] HPO_3 | 1 | 1 | [HPO3] 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 = ([H3PO4])^(-1) [H2O] [HPO3] = ([H2O] [HPO3])/([H3PO4])
Rate of reaction
![Construct the rate of reaction expression for: H_3PO_4 ⟶ H_2O + HPO_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: H_3PO_4 ⟶ H_2O + HPO_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 H_3PO_4 | 1 | -1 H_2O | 1 | 1 HPO_3 | 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_3PO_4 | 1 | -1 | -(Δ[H3PO4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) HPO_3 | 1 | 1 | (Δ[HPO3])/(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[H3PO4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[HPO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/a20b5318454319f423d2152a9b7dc294.png)
Construct the rate of reaction expression for: H_3PO_4 ⟶ H_2O + HPO_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: H_3PO_4 ⟶ H_2O + HPO_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 H_3PO_4 | 1 | -1 H_2O | 1 | 1 HPO_3 | 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_3PO_4 | 1 | -1 | -(Δ[H3PO4])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) HPO_3 | 1 | 1 | (Δ[HPO3])/(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[H3PO4])/(Δt) = (Δ[H2O])/(Δt) = (Δ[HPO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| phosphoric acid | water | metaphosphoric acid formula | H_3PO_4 | H_2O | HPO_3 Hill formula | H_3O_4P | H_2O | HO_3P name | phosphoric acid | water | metaphosphoric acid IUPAC name | phosphoric acid | water | phosphenic acid](../image_source/6d26608ae5d8b878df94a41fd05f3f84.png)
| phosphoric acid | water | metaphosphoric acid formula | H_3PO_4 | H_2O | HPO_3 Hill formula | H_3O_4P | H_2O | HO_3P name | phosphoric acid | water | metaphosphoric acid IUPAC name | phosphoric acid | water | phosphenic acid
Substance properties
![| phosphoric acid | water | metaphosphoric acid molar mass | 97.994 g/mol | 18.015 g/mol | 79.979 g/mol phase | liquid (at STP) | liquid (at STP) | liquid (at STP) melting point | 42.4 °C | 0 °C | 21 °C boiling point | 158 °C | 99.9839 °C | 260 °C density | 1.685 g/cm^3 | 1 g/cm^3 | 2.4 g/cm^3 solubility in water | very soluble | | soluble surface tension | | 0.0728 N/m | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | odorless |](../image_source/aa85844ace6b4681a871f1a182080f03.png)
| phosphoric acid | water | metaphosphoric acid molar mass | 97.994 g/mol | 18.015 g/mol | 79.979 g/mol phase | liquid (at STP) | liquid (at STP) | liquid (at STP) melting point | 42.4 °C | 0 °C | 21 °C boiling point | 158 °C | 99.9839 °C | 260 °C density | 1.685 g/cm^3 | 1 g/cm^3 | 2.4 g/cm^3 solubility in water | very soluble | | soluble surface tension | | 0.0728 N/m | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | odorless |
Units