Input interpretation
![H_2O water + H8B2O2 ⟶ H_2 hydrogen + HBO_2 metaboric acid](../image_source/5619a3b2f88e781537e6cc943f2093fc.png)
H_2O water + H8B2O2 ⟶ H_2 hydrogen + HBO_2 metaboric acid
Balanced equation
![Balance the chemical equation algebraically: H_2O + H8B2O2 ⟶ H_2 + HBO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 H8B2O2 ⟶ c_3 H_2 + c_4 HBO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and B: H: | 2 c_1 + 8 c_2 = 2 c_3 + c_4 O: | c_1 + 2 c_2 = 2 c_4 B: | 2 c_2 = c_4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 5 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + H8B2O2 ⟶ 5 H_2 + 2 HBO_2](../image_source/f5ecb60d63205d5234db3fde46632892.png)
Balance the chemical equation algebraically: H_2O + H8B2O2 ⟶ H_2 + HBO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 H8B2O2 ⟶ c_3 H_2 + c_4 HBO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and B: H: | 2 c_1 + 8 c_2 = 2 c_3 + c_4 O: | c_1 + 2 c_2 = 2 c_4 B: | 2 c_2 = c_4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 5 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + H8B2O2 ⟶ 5 H_2 + 2 HBO_2
Structures
![+ H8B2O2 ⟶ +](../image_source/30d86378e914e2e1cebfa19252e504c0.png)
+ H8B2O2 ⟶ +
Names
![water + H8B2O2 ⟶ hydrogen + metaboric acid](../image_source/e98e7f8a3fc926e44555327256c21ee9.png)
water + H8B2O2 ⟶ hydrogen + metaboric acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2O + H8B2O2 ⟶ H_2 + HBO_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: 2 H_2O + H8B2O2 ⟶ 5 H_2 + 2 HBO_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 H_2O | 2 | -2 H8B2O2 | 1 | -1 H_2 | 5 | 5 HBO_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) H8B2O2 | 1 | -1 | ([H8B2O2])^(-1) H_2 | 5 | 5 | ([H2])^5 HBO_2 | 2 | 2 | ([HBO2])^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 = ([H2O])^(-2) ([H8B2O2])^(-1) ([H2])^5 ([HBO2])^2 = (([H2])^5 ([HBO2])^2)/(([H2O])^2 [H8B2O2])](../image_source/f56f71e427330fb8b03351ca877c97da.png)
Construct the equilibrium constant, K, expression for: H_2O + H8B2O2 ⟶ H_2 + HBO_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: 2 H_2O + H8B2O2 ⟶ 5 H_2 + 2 HBO_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 H_2O | 2 | -2 H8B2O2 | 1 | -1 H_2 | 5 | 5 HBO_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) H8B2O2 | 1 | -1 | ([H8B2O2])^(-1) H_2 | 5 | 5 | ([H2])^5 HBO_2 | 2 | 2 | ([HBO2])^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 = ([H2O])^(-2) ([H8B2O2])^(-1) ([H2])^5 ([HBO2])^2 = (([H2])^5 ([HBO2])^2)/(([H2O])^2 [H8B2O2])
Rate of reaction
![Construct the rate of reaction expression for: H_2O + H8B2O2 ⟶ H_2 + HBO_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: 2 H_2O + H8B2O2 ⟶ 5 H_2 + 2 HBO_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 H_2O | 2 | -2 H8B2O2 | 1 | -1 H_2 | 5 | 5 HBO_2 | 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) H8B2O2 | 1 | -1 | -(Δ[H8B2O2])/(Δt) H_2 | 5 | 5 | 1/5 (Δ[H2])/(Δt) HBO_2 | 2 | 2 | 1/2 (Δ[HBO2])/(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[H2O])/(Δt) = -(Δ[H8B2O2])/(Δt) = 1/5 (Δ[H2])/(Δt) = 1/2 (Δ[HBO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/2511af36c7ca49401ec75fa9289e5263.png)
Construct the rate of reaction expression for: H_2O + H8B2O2 ⟶ H_2 + HBO_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: 2 H_2O + H8B2O2 ⟶ 5 H_2 + 2 HBO_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 H_2O | 2 | -2 H8B2O2 | 1 | -1 H_2 | 5 | 5 HBO_2 | 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) H8B2O2 | 1 | -1 | -(Δ[H8B2O2])/(Δt) H_2 | 5 | 5 | 1/5 (Δ[H2])/(Δt) HBO_2 | 2 | 2 | 1/2 (Δ[HBO2])/(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[H2O])/(Δt) = -(Δ[H8B2O2])/(Δt) = 1/5 (Δ[H2])/(Δt) = 1/2 (Δ[HBO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| water | H8B2O2 | hydrogen | metaboric acid formula | H_2O | H8B2O2 | H_2 | HBO_2 Hill formula | H_2O | H8B2O2 | H_2 | BHO_2 name | water | | hydrogen | metaboric acid IUPAC name | water | | molecular hydrogen | oxoborinic acid](../image_source/c304e0faabd05473f6d83f34f76248ba.png)
| water | H8B2O2 | hydrogen | metaboric acid formula | H_2O | H8B2O2 | H_2 | HBO_2 Hill formula | H_2O | H8B2O2 | H_2 | BHO_2 name | water | | hydrogen | metaboric acid IUPAC name | water | | molecular hydrogen | oxoborinic acid
Substance properties
![| water | H8B2O2 | hydrogen | metaboric acid molar mass | 18.015 g/mol | 61.68 g/mol | 2.016 g/mol | 43.82 g/mol phase | liquid (at STP) | | gas (at STP) | melting point | 0 °C | | -259.2 °C | boiling point | 99.9839 °C | | -252.8 °C | density | 1 g/cm^3 | | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.49 g/cm^3 surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | odorless | | odorless |](../image_source/eb68186a674c6eea72a5415eff97c665.png)
| water | H8B2O2 | hydrogen | metaboric acid molar mass | 18.015 g/mol | 61.68 g/mol | 2.016 g/mol | 43.82 g/mol phase | liquid (at STP) | | gas (at STP) | melting point | 0 °C | | -259.2 °C | boiling point | 99.9839 °C | | -252.8 °C | density | 1 g/cm^3 | | 8.99×10^-5 g/cm^3 (at 0 °C) | 2.49 g/cm^3 surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | odorless | | odorless |
Units