Input interpretation
![N_2 nitrogen + Be beryllium ⟶ Be3N2](../image_source/e3e1b02e7fc78bdc6bff54cb706bcc06.png)
N_2 nitrogen + Be beryllium ⟶ Be3N2
Balanced equation
![Balance the chemical equation algebraically: N_2 + Be ⟶ Be3N2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 N_2 + c_2 Be ⟶ c_3 Be3N2 Set the number of atoms in the reactants equal to the number of atoms in the products for N and Be: N: | 2 c_1 = 2 c_3 Be: | c_2 = 3 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 = 3 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | N_2 + 3 Be ⟶ Be3N2](../image_source/b5655a2ea1afa8d1051487de4bb52d07.png)
Balance the chemical equation algebraically: N_2 + Be ⟶ Be3N2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 N_2 + c_2 Be ⟶ c_3 Be3N2 Set the number of atoms in the reactants equal to the number of atoms in the products for N and Be: N: | 2 c_1 = 2 c_3 Be: | c_2 = 3 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 = 3 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | N_2 + 3 Be ⟶ Be3N2
Structures
![+ ⟶ Be3N2](../image_source/e5051551bcb38ff16ede0a561b854a57.png)
+ ⟶ Be3N2
Names
![nitrogen + beryllium ⟶ Be3N2](../image_source/7ed72984f79f227dfac3895dbb7bb285.png)
nitrogen + beryllium ⟶ Be3N2
Equilibrium constant
![Construct the equilibrium constant, K, expression for: N_2 + Be ⟶ Be3N2 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: N_2 + 3 Be ⟶ Be3N2 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 N_2 | 1 | -1 Be | 3 | -3 Be3N2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression N_2 | 1 | -1 | ([N2])^(-1) Be | 3 | -3 | ([Be])^(-3) Be3N2 | 1 | 1 | [Be3N2] 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 = ([N2])^(-1) ([Be])^(-3) [Be3N2] = ([Be3N2])/([N2] ([Be])^3)](../image_source/c1360ac563733a2c08d9f4d800f11fd1.png)
Construct the equilibrium constant, K, expression for: N_2 + Be ⟶ Be3N2 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: N_2 + 3 Be ⟶ Be3N2 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 N_2 | 1 | -1 Be | 3 | -3 Be3N2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression N_2 | 1 | -1 | ([N2])^(-1) Be | 3 | -3 | ([Be])^(-3) Be3N2 | 1 | 1 | [Be3N2] 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 = ([N2])^(-1) ([Be])^(-3) [Be3N2] = ([Be3N2])/([N2] ([Be])^3)
Rate of reaction
![Construct the rate of reaction expression for: N_2 + Be ⟶ Be3N2 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: N_2 + 3 Be ⟶ Be3N2 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 N_2 | 1 | -1 Be | 3 | -3 Be3N2 | 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 N_2 | 1 | -1 | -(Δ[N2])/(Δt) Be | 3 | -3 | -1/3 (Δ[Be])/(Δt) Be3N2 | 1 | 1 | (Δ[Be3N2])/(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[N2])/(Δt) = -1/3 (Δ[Be])/(Δt) = (Δ[Be3N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/bb9757d97d72285a7d276258af890474.png)
Construct the rate of reaction expression for: N_2 + Be ⟶ Be3N2 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: N_2 + 3 Be ⟶ Be3N2 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 N_2 | 1 | -1 Be | 3 | -3 Be3N2 | 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 N_2 | 1 | -1 | -(Δ[N2])/(Δt) Be | 3 | -3 | -1/3 (Δ[Be])/(Δt) Be3N2 | 1 | 1 | (Δ[Be3N2])/(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[N2])/(Δt) = -1/3 (Δ[Be])/(Δt) = (Δ[Be3N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| nitrogen | beryllium | Be3N2 formula | N_2 | Be | Be3N2 name | nitrogen | beryllium | IUPAC name | molecular nitrogen | beryllium |](../image_source/89a69913b5965c438af57ac6a24768d0.png)
| nitrogen | beryllium | Be3N2 formula | N_2 | Be | Be3N2 name | nitrogen | beryllium | IUPAC name | molecular nitrogen | beryllium |
Substance properties
![| nitrogen | beryllium | Be3N2 molar mass | 28.014 g/mol | 9.0121831 g/mol | 55.051 g/mol phase | gas (at STP) | solid (at STP) | melting point | -210 °C | 1278 °C | boiling point | -195.79 °C | 2970 °C | density | 0.001251 g/cm^3 (at 0 °C) | 1.85 g/cm^3 | solubility in water | insoluble | insoluble | surface tension | 0.0066 N/m | | dynamic viscosity | 1.78×10^-5 Pa s (at 25 °C) | | odor | odorless | |](../image_source/d5b365994d95449e2dfaadd371c59eef.png)
| nitrogen | beryllium | Be3N2 molar mass | 28.014 g/mol | 9.0121831 g/mol | 55.051 g/mol phase | gas (at STP) | solid (at STP) | melting point | -210 °C | 1278 °C | boiling point | -195.79 °C | 2970 °C | density | 0.001251 g/cm^3 (at 0 °C) | 1.85 g/cm^3 | solubility in water | insoluble | insoluble | surface tension | 0.0066 N/m | | dynamic viscosity | 1.78×10^-5 Pa s (at 25 °C) | | odor | odorless | |
Units