Input interpretation
![Be(ClO3)2 ⟶ O_2 oxygen + BeCl_2 beryllium chloride](../image_source/de1d3ae4ce84c2c483f230195ae81a0d.png)
Be(ClO3)2 ⟶ O_2 oxygen + BeCl_2 beryllium chloride
Balanced equation
![Balance the chemical equation algebraically: Be(ClO3)2 ⟶ O_2 + BeCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Be(ClO3)2 ⟶ c_2 O_2 + c_3 BeCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Be, Cl and O: Be: | c_1 = c_3 Cl: | 2 c_1 = 2 c_3 O: | 6 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 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Be(ClO3)2 ⟶ 3 O_2 + BeCl_2](../image_source/7593d72ce126a0ccdc37d10ae8eebca8.png)
Balance the chemical equation algebraically: Be(ClO3)2 ⟶ O_2 + BeCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Be(ClO3)2 ⟶ c_2 O_2 + c_3 BeCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Be, Cl and O: Be: | c_1 = c_3 Cl: | 2 c_1 = 2 c_3 O: | 6 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 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Be(ClO3)2 ⟶ 3 O_2 + BeCl_2
Structures
![Be(ClO3)2 ⟶ +](../image_source/346a2ab9f25330b7c4b993ee97da4330.png)
Be(ClO3)2 ⟶ +
Names
![Be(ClO3)2 ⟶ oxygen + beryllium chloride](../image_source/7ee5dbe823adb4ca147057830327bee4.png)
Be(ClO3)2 ⟶ oxygen + beryllium chloride
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Be(ClO3)2 ⟶ O_2 + BeCl_2 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: Be(ClO3)2 ⟶ 3 O_2 + BeCl_2 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 Be(ClO3)2 | 1 | -1 O_2 | 3 | 3 BeCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Be(ClO3)2 | 1 | -1 | ([Be(ClO3)2])^(-1) O_2 | 3 | 3 | ([O2])^3 BeCl_2 | 1 | 1 | [BeCl2] 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 = ([Be(ClO3)2])^(-1) ([O2])^3 [BeCl2] = (([O2])^3 [BeCl2])/([Be(ClO3)2])](../image_source/ee0eccad872820f706cd6dfa25079680.png)
Construct the equilibrium constant, K, expression for: Be(ClO3)2 ⟶ O_2 + BeCl_2 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: Be(ClO3)2 ⟶ 3 O_2 + BeCl_2 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 Be(ClO3)2 | 1 | -1 O_2 | 3 | 3 BeCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Be(ClO3)2 | 1 | -1 | ([Be(ClO3)2])^(-1) O_2 | 3 | 3 | ([O2])^3 BeCl_2 | 1 | 1 | [BeCl2] 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 = ([Be(ClO3)2])^(-1) ([O2])^3 [BeCl2] = (([O2])^3 [BeCl2])/([Be(ClO3)2])
Rate of reaction
![Construct the rate of reaction expression for: Be(ClO3)2 ⟶ O_2 + BeCl_2 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: Be(ClO3)2 ⟶ 3 O_2 + BeCl_2 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 Be(ClO3)2 | 1 | -1 O_2 | 3 | 3 BeCl_2 | 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 Be(ClO3)2 | 1 | -1 | -(Δ[Be(ClO3)2])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) BeCl_2 | 1 | 1 | (Δ[BeCl2])/(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[Be(ClO3)2])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[BeCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/abf142425aa2dc18bb53263012393cdd.png)
Construct the rate of reaction expression for: Be(ClO3)2 ⟶ O_2 + BeCl_2 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: Be(ClO3)2 ⟶ 3 O_2 + BeCl_2 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 Be(ClO3)2 | 1 | -1 O_2 | 3 | 3 BeCl_2 | 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 Be(ClO3)2 | 1 | -1 | -(Δ[Be(ClO3)2])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) BeCl_2 | 1 | 1 | (Δ[BeCl2])/(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[Be(ClO3)2])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[BeCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| Be(ClO3)2 | oxygen | beryllium chloride formula | Be(ClO3)2 | O_2 | BeCl_2 Hill formula | BeCl2O6 | O_2 | BeCl_2 name | | oxygen | beryllium chloride IUPAC name | | molecular oxygen | beryllium dichloride](../image_source/30132759a2d66aa21dd442f3f1e7a6aa.png)
| Be(ClO3)2 | oxygen | beryllium chloride formula | Be(ClO3)2 | O_2 | BeCl_2 Hill formula | BeCl2O6 | O_2 | BeCl_2 name | | oxygen | beryllium chloride IUPAC name | | molecular oxygen | beryllium dichloride
Substance properties
![| Be(ClO3)2 | oxygen | beryllium chloride molar mass | 175.9 g/mol | 31.998 g/mol | 79.91 g/mol phase | | gas (at STP) | solid (at STP) melting point | | -218 °C | 399 °C boiling point | | -183 °C | 500 °C density | | 0.001429 g/cm^3 (at 0 °C) | 1.899 g/cm^3 surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless |](../image_source/c8de2c4ab5414ac05ebf2493d496e942.png)
| Be(ClO3)2 | oxygen | beryllium chloride molar mass | 175.9 g/mol | 31.998 g/mol | 79.91 g/mol phase | | gas (at STP) | solid (at STP) melting point | | -218 °C | 399 °C boiling point | | -183 °C | 500 °C density | | 0.001429 g/cm^3 (at 0 °C) | 1.899 g/cm^3 surface tension | | 0.01347 N/m | dynamic viscosity | | 2.055×10^-5 Pa s (at 25 °C) | odor | | odorless |
Units