Input interpretation
![AsH_3 arsine ⟶ H_2 hydrogen + As gray arsenic](../image_source/caff3ee3e00673a48907dacce18d1a5e.png)
AsH_3 arsine ⟶ H_2 hydrogen + As gray arsenic
Balanced equation
![Balance the chemical equation algebraically: AsH_3 ⟶ H_2 + As Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AsH_3 ⟶ c_2 H_2 + c_3 As Set the number of atoms in the reactants equal to the number of atoms in the products for As and H: As: | c_1 = c_3 H: | 3 c_1 = 2 c_2 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 = 3/2 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AsH_3 ⟶ 3 H_2 + 2 As](../image_source/3a84e65647d6bb3f2d23ead31f051e81.png)
Balance the chemical equation algebraically: AsH_3 ⟶ H_2 + As Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AsH_3 ⟶ c_2 H_2 + c_3 As Set the number of atoms in the reactants equal to the number of atoms in the products for As and H: As: | c_1 = c_3 H: | 3 c_1 = 2 c_2 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 = 3/2 c_3 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AsH_3 ⟶ 3 H_2 + 2 As
Structures
![⟶ +](../image_source/d8f2172eea72d85367f2f8237e1f67f6.png)
⟶ +
Names
![arsine ⟶ hydrogen + gray arsenic](../image_source/fcd3d370e5111077d439f1e15f1f9815.png)
arsine ⟶ hydrogen + gray arsenic
Reaction thermodynamics
Enthalpy
![| arsine | hydrogen | gray arsenic molecular enthalpy | 66.4 kJ/mol | 0 kJ/mol | 0 kJ/mol total enthalpy | 132.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | H_initial = 132.8 kJ/mol | H_final = 0 kJ/mol | ΔH_rxn^0 | 0 kJ/mol - 132.8 kJ/mol = -132.8 kJ/mol (exothermic) | |](../image_source/6d35beb1c93299d4e6b84087d9e0c429.png)
| arsine | hydrogen | gray arsenic molecular enthalpy | 66.4 kJ/mol | 0 kJ/mol | 0 kJ/mol total enthalpy | 132.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | H_initial = 132.8 kJ/mol | H_final = 0 kJ/mol | ΔH_rxn^0 | 0 kJ/mol - 132.8 kJ/mol = -132.8 kJ/mol (exothermic) | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: AsH_3 ⟶ H_2 + As 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 AsH_3 ⟶ 3 H_2 + 2 As 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 AsH_3 | 2 | -2 H_2 | 3 | 3 As | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AsH_3 | 2 | -2 | ([AsH3])^(-2) H_2 | 3 | 3 | ([H2])^3 As | 2 | 2 | ([As])^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 = ([AsH3])^(-2) ([H2])^3 ([As])^2 = (([H2])^3 ([As])^2)/([AsH3])^2](../image_source/fb6378b5655335a1e0491a3b57db7799.png)
Construct the equilibrium constant, K, expression for: AsH_3 ⟶ H_2 + As 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 AsH_3 ⟶ 3 H_2 + 2 As 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 AsH_3 | 2 | -2 H_2 | 3 | 3 As | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AsH_3 | 2 | -2 | ([AsH3])^(-2) H_2 | 3 | 3 | ([H2])^3 As | 2 | 2 | ([As])^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 = ([AsH3])^(-2) ([H2])^3 ([As])^2 = (([H2])^3 ([As])^2)/([AsH3])^2
Rate of reaction
![Construct the rate of reaction expression for: AsH_3 ⟶ H_2 + As 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 AsH_3 ⟶ 3 H_2 + 2 As 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 AsH_3 | 2 | -2 H_2 | 3 | 3 As | 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 AsH_3 | 2 | -2 | -1/2 (Δ[AsH3])/(Δt) H_2 | 3 | 3 | 1/3 (Δ[H2])/(Δt) As | 2 | 2 | 1/2 (Δ[As])/(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[AsH3])/(Δt) = 1/3 (Δ[H2])/(Δt) = 1/2 (Δ[As])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/bc11f4d35e1c5d835b74e36e8be6954d.png)
Construct the rate of reaction expression for: AsH_3 ⟶ H_2 + As 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 AsH_3 ⟶ 3 H_2 + 2 As 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 AsH_3 | 2 | -2 H_2 | 3 | 3 As | 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 AsH_3 | 2 | -2 | -1/2 (Δ[AsH3])/(Δt) H_2 | 3 | 3 | 1/3 (Δ[H2])/(Δt) As | 2 | 2 | 1/2 (Δ[As])/(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[AsH3])/(Δt) = 1/3 (Δ[H2])/(Δt) = 1/2 (Δ[As])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| arsine | hydrogen | gray arsenic formula | AsH_3 | H_2 | As name | arsine | hydrogen | gray arsenic IUPAC name | arsane | molecular hydrogen | arsenic](../image_source/76b4e77aed086ad15b3ebf0997d2f2c8.png)
| arsine | hydrogen | gray arsenic formula | AsH_3 | H_2 | As name | arsine | hydrogen | gray arsenic IUPAC name | arsane | molecular hydrogen | arsenic
Substance properties
![| arsine | hydrogen | gray arsenic molar mass | 77.946 g/mol | 2.016 g/mol | 74.921595 g/mol phase | gas (at STP) | gas (at STP) | solid (at STP) melting point | -111.2 °C | -259.2 °C | 817 °C boiling point | -62.5 °C | -252.8 °C | 616 °C density | 0.003186 g/cm^3 (at 25 °C) | 8.99×10^-5 g/cm^3 (at 0 °C) | 5.727 g/cm^3 solubility in water | | | insoluble dynamic viscosity | 1.47×10^-5 Pa s (at 0 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | | odorless | odorless](../image_source/0cad39079756606b6f143554577644a9.png)
| arsine | hydrogen | gray arsenic molar mass | 77.946 g/mol | 2.016 g/mol | 74.921595 g/mol phase | gas (at STP) | gas (at STP) | solid (at STP) melting point | -111.2 °C | -259.2 °C | 817 °C boiling point | -62.5 °C | -252.8 °C | 616 °C density | 0.003186 g/cm^3 (at 25 °C) | 8.99×10^-5 g/cm^3 (at 0 °C) | 5.727 g/cm^3 solubility in water | | | insoluble dynamic viscosity | 1.47×10^-5 Pa s (at 0 °C) | 8.9×10^-6 Pa s (at 25 °C) | odor | | odorless | odorless
Units