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KOH + MgO = Mg(OH)2 + K2O

Input interpretation

KOH potassium hydroxide + MgO magnesium oxide ⟶ Mg(OH)_2 magnesium hydroxide + K_2O potassium oxide
KOH potassium hydroxide + MgO magnesium oxide ⟶ Mg(OH)_2 magnesium hydroxide + K_2O potassium oxide

Balanced equation

Balance the chemical equation algebraically: KOH + MgO ⟶ Mg(OH)_2 + K_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 MgO ⟶ c_3 Mg(OH)_2 + c_4 K_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and Mg: H: | c_1 = 2 c_3 K: | c_1 = 2 c_4 O: | c_1 + c_2 = 2 c_3 + c_4 Mg: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + MgO ⟶ Mg(OH)_2 + K_2O
Balance the chemical equation algebraically: KOH + MgO ⟶ Mg(OH)_2 + K_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 MgO ⟶ c_3 Mg(OH)_2 + c_4 K_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and Mg: H: | c_1 = 2 c_3 K: | c_1 = 2 c_4 O: | c_1 + c_2 = 2 c_3 + c_4 Mg: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + MgO ⟶ Mg(OH)_2 + K_2O

Structures

+ ⟶ +
+ ⟶ +

Names

potassium hydroxide + magnesium oxide ⟶ magnesium hydroxide + potassium oxide
potassium hydroxide + magnesium oxide ⟶ magnesium hydroxide + potassium oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH | 2 | -2 MgO | 1 | -1 Mg(OH)_2 | 1 | 1 K_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) MgO | 1 | -1 | ([MgO])^(-1) Mg(OH)_2 | 1 | 1 | [Mg(OH)2] K_2O | 1 | 1 | [K2O] 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 = ([KOH])^(-2) ([MgO])^(-1) [Mg(OH)2] [K2O] = ([Mg(OH)2] [K2O])/(([KOH])^2 [MgO])
Construct the equilibrium constant, K, expression for: KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH | 2 | -2 MgO | 1 | -1 Mg(OH)_2 | 1 | 1 K_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) MgO | 1 | -1 | ([MgO])^(-1) Mg(OH)_2 | 1 | 1 | [Mg(OH)2] K_2O | 1 | 1 | [K2O] 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 = ([KOH])^(-2) ([MgO])^(-1) [Mg(OH)2] [K2O] = ([Mg(OH)2] [K2O])/(([KOH])^2 [MgO])

Rate of reaction

Construct the rate of reaction expression for: KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH | 2 | -2 MgO | 1 | -1 Mg(OH)_2 | 1 | 1 K_2O | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) MgO | 1 | -1 | -(Δ[MgO])/(Δt) Mg(OH)_2 | 1 | 1 | (Δ[Mg(OH)2])/(Δt) K_2O | 1 | 1 | (Δ[K2O])/(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[KOH])/(Δt) = -(Δ[MgO])/(Δt) = (Δ[Mg(OH)2])/(Δt) = (Δ[K2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH + MgO ⟶ Mg(OH)_2 + K_2O 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 KOH | 2 | -2 MgO | 1 | -1 Mg(OH)_2 | 1 | 1 K_2O | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) MgO | 1 | -1 | -(Δ[MgO])/(Δt) Mg(OH)_2 | 1 | 1 | (Δ[Mg(OH)2])/(Δt) K_2O | 1 | 1 | (Δ[K2O])/(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[KOH])/(Δt) = -(Δ[MgO])/(Δt) = (Δ[Mg(OH)2])/(Δt) = (Δ[K2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | magnesium oxide | magnesium hydroxide | potassium oxide formula | KOH | MgO | Mg(OH)_2 | K_2O Hill formula | HKO | MgO | H_2MgO_2 | K_2O name | potassium hydroxide | magnesium oxide | magnesium hydroxide | potassium oxide IUPAC name | potassium hydroxide | oxomagnesium | magnesium dihydroxide | dipotassium oxygen(2-)
| potassium hydroxide | magnesium oxide | magnesium hydroxide | potassium oxide formula | KOH | MgO | Mg(OH)_2 | K_2O Hill formula | HKO | MgO | H_2MgO_2 | K_2O name | potassium hydroxide | magnesium oxide | magnesium hydroxide | potassium oxide IUPAC name | potassium hydroxide | oxomagnesium | magnesium dihydroxide | dipotassium oxygen(2-)

Substance properties

| potassium hydroxide | magnesium oxide | magnesium hydroxide | potassium oxide molar mass | 56.105 g/mol | 40.304 g/mol | 58.319 g/mol | 94.196 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 406 °C | 2852 °C | 350 °C | boiling point | 1327 °C | 3600 °C | | density | 2.044 g/cm^3 | 3.58 g/cm^3 | 2.3446 g/cm^3 | solubility in water | soluble | | insoluble | dynamic viscosity | 0.001 Pa s (at 550 °C) | | | odor | | odorless | |
| potassium hydroxide | magnesium oxide | magnesium hydroxide | potassium oxide molar mass | 56.105 g/mol | 40.304 g/mol | 58.319 g/mol | 94.196 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 406 °C | 2852 °C | 350 °C | boiling point | 1327 °C | 3600 °C | | density | 2.044 g/cm^3 | 3.58 g/cm^3 | 2.3446 g/cm^3 | solubility in water | soluble | | insoluble | dynamic viscosity | 0.001 Pa s (at 550 °C) | | | odor | | odorless | |

Units

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