Input interpretation
H_2 hydrogen + SbF7 ⟶ H2SbF7
Balanced equation
Balance the chemical equation algebraically: H_2 + SbF7 ⟶ H2SbF7 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 SbF7 ⟶ c_3 H2SbF7 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Sb and F: H: | 2 c_1 = 2 c_3 Sb: | c_2 = c_3 F: | 7 c_2 = 7 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_2 + SbF7 ⟶ H2SbF7
Structures
+ SbF7 ⟶ H2SbF7
Names
hydrogen + SbF7 ⟶ H2SbF7
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2 + SbF7 ⟶ H2SbF7 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 + SbF7 ⟶ H2SbF7 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 SbF7 | 1 | -1 H2SbF7 | 1 | 1 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) SbF7 | 1 | -1 | ([SbF7])^(-1) H2SbF7 | 1 | 1 | [H2SbF7] 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) ([SbF7])^(-1) [H2SbF7] = ([H2SbF7])/([H2] [SbF7])](../image_source/0fabf546ad9693f968760d0c02dccae1.png)
Construct the equilibrium constant, K, expression for: H_2 + SbF7 ⟶ H2SbF7 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 + SbF7 ⟶ H2SbF7 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 SbF7 | 1 | -1 H2SbF7 | 1 | 1 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) SbF7 | 1 | -1 | ([SbF7])^(-1) H2SbF7 | 1 | 1 | [H2SbF7] 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) ([SbF7])^(-1) [H2SbF7] = ([H2SbF7])/([H2] [SbF7])
Rate of reaction
![Construct the rate of reaction expression for: H_2 + SbF7 ⟶ H2SbF7 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 + SbF7 ⟶ H2SbF7 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 SbF7 | 1 | -1 H2SbF7 | 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_2 | 1 | -1 | -(Δ[H2])/(Δt) SbF7 | 1 | -1 | -(Δ[SbF7])/(Δt) H2SbF7 | 1 | 1 | (Δ[H2SbF7])/(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) = -(Δ[SbF7])/(Δt) = (Δ[H2SbF7])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/4f4d594da4eeffdf5125e89fb0a1b6a7.png)
Construct the rate of reaction expression for: H_2 + SbF7 ⟶ H2SbF7 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 + SbF7 ⟶ H2SbF7 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 SbF7 | 1 | -1 H2SbF7 | 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_2 | 1 | -1 | -(Δ[H2])/(Δt) SbF7 | 1 | -1 | -(Δ[SbF7])/(Δt) H2SbF7 | 1 | 1 | (Δ[H2SbF7])/(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) = -(Δ[SbF7])/(Δt) = (Δ[H2SbF7])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| hydrogen | SbF7 | H2SbF7 formula | H_2 | SbF7 | H2SbF7 Hill formula | H_2 | F7Sb | H2F7Sb name | hydrogen | | IUPAC name | molecular hydrogen | |
Substance properties
| hydrogen | SbF7 | H2SbF7 molar mass | 2.016 g/mol | 254.749 g/mol | 256.765 g/mol phase | gas (at STP) | | melting point | -259.2 °C | | boiling point | -252.8 °C | | density | 8.99×10^-5 g/cm^3 (at 0 °C) | | dynamic viscosity | 8.9×10^-6 Pa s (at 25 °C) | | odor | odorless | |
Units
