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H2O + K2SO4 = H2SO4 + KOH

Input interpretation

H_2O water + K_2SO_4 potassium sulfate ⟶ H_2SO_4 sulfuric acid + KOH potassium hydroxide
H_2O water + K_2SO_4 potassium sulfate ⟶ H_2SO_4 sulfuric acid + KOH potassium hydroxide

Balanced equation

Balance the chemical equation algebraically: H_2O + K_2SO_4 ⟶ H_2SO_4 + KOH Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 K_2SO_4 ⟶ c_3 H_2SO_4 + c_4 KOH Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K and S: H: | 2 c_1 = 2 c_3 + c_4 O: | c_1 + 4 c_2 = 4 c_3 + c_4 K: | 2 c_2 = c_4 S: | 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + K_2SO_4 ⟶ H_2SO_4 + 2 KOH
Balance the chemical equation algebraically: H_2O + K_2SO_4 ⟶ H_2SO_4 + KOH Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 K_2SO_4 ⟶ c_3 H_2SO_4 + c_4 KOH Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K and S: H: | 2 c_1 = 2 c_3 + c_4 O: | c_1 + 4 c_2 = 4 c_3 + c_4 K: | 2 c_2 = c_4 S: | 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + K_2SO_4 ⟶ H_2SO_4 + 2 KOH

Structures

+ ⟶ +
+ ⟶ +

Names

water + potassium sulfate ⟶ sulfuric acid + potassium hydroxide
water + potassium sulfate ⟶ sulfuric acid + potassium hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + K_2SO_4 ⟶ H_2SO_4 + KOH 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 + K_2SO_4 ⟶ H_2SO_4 + 2 KOH 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 K_2SO_4 | 1 | -1 H_2SO_4 | 1 | 1 KOH | 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) K_2SO_4 | 1 | -1 | ([K2SO4])^(-1) H_2SO_4 | 1 | 1 | [H2SO4] KOH | 2 | 2 | ([KOH])^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) ([K2SO4])^(-1) [H2SO4] ([KOH])^2 = ([H2SO4] ([KOH])^2)/(([H2O])^2 [K2SO4])
Construct the equilibrium constant, K, expression for: H_2O + K_2SO_4 ⟶ H_2SO_4 + KOH 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 + K_2SO_4 ⟶ H_2SO_4 + 2 KOH 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 K_2SO_4 | 1 | -1 H_2SO_4 | 1 | 1 KOH | 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) K_2SO_4 | 1 | -1 | ([K2SO4])^(-1) H_2SO_4 | 1 | 1 | [H2SO4] KOH | 2 | 2 | ([KOH])^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) ([K2SO4])^(-1) [H2SO4] ([KOH])^2 = ([H2SO4] ([KOH])^2)/(([H2O])^2 [K2SO4])

Rate of reaction

Construct the rate of reaction expression for: H_2O + K_2SO_4 ⟶ H_2SO_4 + KOH 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 + K_2SO_4 ⟶ H_2SO_4 + 2 KOH 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 K_2SO_4 | 1 | -1 H_2SO_4 | 1 | 1 KOH | 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) K_2SO_4 | 1 | -1 | -(Δ[K2SO4])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(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[K2SO4])/(Δt) = (Δ[H2SO4])/(Δt) = 1/2 (Δ[KOH])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + K_2SO_4 ⟶ H_2SO_4 + KOH 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 + K_2SO_4 ⟶ H_2SO_4 + 2 KOH 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 K_2SO_4 | 1 | -1 H_2SO_4 | 1 | 1 KOH | 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) K_2SO_4 | 1 | -1 | -(Δ[K2SO4])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(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[K2SO4])/(Δt) = (Δ[H2SO4])/(Δt) = 1/2 (Δ[KOH])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | potassium sulfate | sulfuric acid | potassium hydroxide formula | H_2O | K_2SO_4 | H_2SO_4 | KOH Hill formula | H_2O | K_2O_4S | H_2O_4S | HKO name | water | potassium sulfate | sulfuric acid | potassium hydroxide IUPAC name | water | dipotassium sulfate | sulfuric acid | potassium hydroxide
| water | potassium sulfate | sulfuric acid | potassium hydroxide formula | H_2O | K_2SO_4 | H_2SO_4 | KOH Hill formula | H_2O | K_2O_4S | H_2O_4S | HKO name | water | potassium sulfate | sulfuric acid | potassium hydroxide IUPAC name | water | dipotassium sulfate | sulfuric acid | potassium hydroxide

Substance properties

| water | potassium sulfate | sulfuric acid | potassium hydroxide molar mass | 18.015 g/mol | 174.25 g/mol | 98.07 g/mol | 56.105 g/mol phase | liquid (at STP) | | liquid (at STP) | solid (at STP) melting point | 0 °C | | 10.371 °C | 406 °C boiling point | 99.9839 °C | | 279.6 °C | 1327 °C density | 1 g/cm^3 | | 1.8305 g/cm^3 | 2.044 g/cm^3 solubility in water | | soluble | very soluble | soluble surface tension | 0.0728 N/m | | 0.0735 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) odor | odorless | | odorless |
| water | potassium sulfate | sulfuric acid | potassium hydroxide molar mass | 18.015 g/mol | 174.25 g/mol | 98.07 g/mol | 56.105 g/mol phase | liquid (at STP) | | liquid (at STP) | solid (at STP) melting point | 0 °C | | 10.371 °C | 406 °C boiling point | 99.9839 °C | | 279.6 °C | 1327 °C density | 1 g/cm^3 | | 1.8305 g/cm^3 | 2.044 g/cm^3 solubility in water | | soluble | very soluble | soluble surface tension | 0.0728 N/m | | 0.0735 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) odor | odorless | | odorless |

Units

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