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O2 + KOH + Ge = H2O + K2GeO3

Input interpretation

O_2 oxygen + KOH potassium hydroxide + Ge germanium ⟶ H_2O water + K2GeO3
O_2 oxygen + KOH potassium hydroxide + Ge germanium ⟶ H_2O water + K2GeO3

Balanced equation

Balance the chemical equation algebraically: O_2 + KOH + Ge ⟶ H_2O + K2GeO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 KOH + c_3 Ge ⟶ c_4 H_2O + c_5 K2GeO3 Set the number of atoms in the reactants equal to the number of atoms in the products for O, H, K and Ge: O: | 2 c_1 + c_2 = c_4 + 3 c_5 H: | c_2 = 2 c_4 K: | c_2 = 2 c_5 Ge: | c_3 = c_5 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 = 2 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | O_2 + 2 KOH + Ge ⟶ H_2O + K2GeO3
Balance the chemical equation algebraically: O_2 + KOH + Ge ⟶ H_2O + K2GeO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 KOH + c_3 Ge ⟶ c_4 H_2O + c_5 K2GeO3 Set the number of atoms in the reactants equal to the number of atoms in the products for O, H, K and Ge: O: | 2 c_1 + c_2 = c_4 + 3 c_5 H: | c_2 = 2 c_4 K: | c_2 = 2 c_5 Ge: | c_3 = c_5 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 = 2 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | O_2 + 2 KOH + Ge ⟶ H_2O + K2GeO3

Structures

+ + ⟶ + K2GeO3
+ + ⟶ + K2GeO3

Names

oxygen + potassium hydroxide + germanium ⟶ water + K2GeO3
oxygen + potassium hydroxide + germanium ⟶ water + K2GeO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: O_2 + KOH + Ge ⟶ H_2O + K2GeO3 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: O_2 + 2 KOH + Ge ⟶ H_2O + K2GeO3 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 O_2 | 1 | -1 KOH | 2 | -2 Ge | 1 | -1 H_2O | 1 | 1 K2GeO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 1 | -1 | ([O2])^(-1) KOH | 2 | -2 | ([KOH])^(-2) Ge | 1 | -1 | ([Ge])^(-1) H_2O | 1 | 1 | [H2O] K2GeO3 | 1 | 1 | [K2GeO3] 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 = ([O2])^(-1) ([KOH])^(-2) ([Ge])^(-1) [H2O] [K2GeO3] = ([H2O] [K2GeO3])/([O2] ([KOH])^2 [Ge])
Construct the equilibrium constant, K, expression for: O_2 + KOH + Ge ⟶ H_2O + K2GeO3 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: O_2 + 2 KOH + Ge ⟶ H_2O + K2GeO3 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 O_2 | 1 | -1 KOH | 2 | -2 Ge | 1 | -1 H_2O | 1 | 1 K2GeO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 1 | -1 | ([O2])^(-1) KOH | 2 | -2 | ([KOH])^(-2) Ge | 1 | -1 | ([Ge])^(-1) H_2O | 1 | 1 | [H2O] K2GeO3 | 1 | 1 | [K2GeO3] 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 = ([O2])^(-1) ([KOH])^(-2) ([Ge])^(-1) [H2O] [K2GeO3] = ([H2O] [K2GeO3])/([O2] ([KOH])^2 [Ge])

Rate of reaction

Construct the rate of reaction expression for: O_2 + KOH + Ge ⟶ H_2O + K2GeO3 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: O_2 + 2 KOH + Ge ⟶ H_2O + K2GeO3 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 O_2 | 1 | -1 KOH | 2 | -2 Ge | 1 | -1 H_2O | 1 | 1 K2GeO3 | 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 O_2 | 1 | -1 | -(Δ[O2])/(Δt) KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) Ge | 1 | -1 | -(Δ[Ge])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K2GeO3 | 1 | 1 | (Δ[K2GeO3])/(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[O2])/(Δt) = -1/2 (Δ[KOH])/(Δt) = -(Δ[Ge])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2GeO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: O_2 + KOH + Ge ⟶ H_2O + K2GeO3 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: O_2 + 2 KOH + Ge ⟶ H_2O + K2GeO3 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 O_2 | 1 | -1 KOH | 2 | -2 Ge | 1 | -1 H_2O | 1 | 1 K2GeO3 | 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 O_2 | 1 | -1 | -(Δ[O2])/(Δt) KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) Ge | 1 | -1 | -(Δ[Ge])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K2GeO3 | 1 | 1 | (Δ[K2GeO3])/(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[O2])/(Δt) = -1/2 (Δ[KOH])/(Δt) = -(Δ[Ge])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2GeO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| oxygen | potassium hydroxide | germanium | water | K2GeO3 formula | O_2 | KOH | Ge | H_2O | K2GeO3 Hill formula | O_2 | HKO | Ge | H_2O | GeK2O3 name | oxygen | potassium hydroxide | germanium | water | IUPAC name | molecular oxygen | potassium hydroxide | germanium | water |
| oxygen | potassium hydroxide | germanium | water | K2GeO3 formula | O_2 | KOH | Ge | H_2O | K2GeO3 Hill formula | O_2 | HKO | Ge | H_2O | GeK2O3 name | oxygen | potassium hydroxide | germanium | water | IUPAC name | molecular oxygen | potassium hydroxide | germanium | water |

Substance properties

| oxygen | potassium hydroxide | germanium | water | K2GeO3 molar mass | 31.998 g/mol | 56.105 g/mol | 72.63 g/mol | 18.015 g/mol | 198.82 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | melting point | -218 °C | 406 °C | 937 °C | 0 °C | boiling point | -183 °C | 1327 °C | 2830 °C | 99.9839 °C | density | 0.001429 g/cm^3 (at 0 °C) | 2.044 g/cm^3 | 5.35 g/cm^3 | 1 g/cm^3 | solubility in water | | soluble | | | surface tension | 0.01347 N/m | | | 0.0728 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | | odorless |
| oxygen | potassium hydroxide | germanium | water | K2GeO3 molar mass | 31.998 g/mol | 56.105 g/mol | 72.63 g/mol | 18.015 g/mol | 198.82 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) | melting point | -218 °C | 406 °C | 937 °C | 0 °C | boiling point | -183 °C | 1327 °C | 2830 °C | 99.9839 °C | density | 0.001429 g/cm^3 (at 0 °C) | 2.044 g/cm^3 | 5.35 g/cm^3 | 1 g/cm^3 | solubility in water | | soluble | | | surface tension | 0.01347 N/m | | | 0.0728 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | | odorless |

Units

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