Input interpretation
![H_2O water + K_2SO_3 potassium sulfite ⟶ KOH potassium hydroxide + KHSO3](../image_source/3aed1a9406328cdceafe4c81e879eb04.png)
H_2O water + K_2SO_3 potassium sulfite ⟶ KOH potassium hydroxide + KHSO3
Balanced equation
![Balance the chemical equation algebraically: H_2O + K_2SO_3 ⟶ KOH + KHSO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 K_2SO_3 ⟶ c_3 KOH + c_4 KHSO3 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 = c_3 + c_4 O: | c_1 + 3 c_2 = c_3 + 3 c_4 K: | 2 c_2 = c_3 + c_4 S: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + K_2SO_3 ⟶ KOH + KHSO3](../image_source/f7d5340d7161ae44998a9950849d33da.png)
Balance the chemical equation algebraically: H_2O + K_2SO_3 ⟶ KOH + KHSO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 K_2SO_3 ⟶ c_3 KOH + c_4 KHSO3 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 = c_3 + c_4 O: | c_1 + 3 c_2 = c_3 + 3 c_4 K: | 2 c_2 = c_3 + c_4 S: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + K_2SO_3 ⟶ KOH + KHSO3
Structures
![+ ⟶ + KHSO3](../image_source/42e4d572e6aea3fb28baaa92850b2068.png)
+ ⟶ + KHSO3
Names
![water + potassium sulfite ⟶ potassium hydroxide + KHSO3](../image_source/fe176ec24c44042ac135fee69615916d.png)
water + potassium sulfite ⟶ potassium hydroxide + KHSO3
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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 | 1 | -1 K_2SO_3 | 1 | -1 KOH | 1 | 1 KHSO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) K_2SO_3 | 1 | -1 | ([K2SO3])^(-1) KOH | 1 | 1 | [KOH] KHSO3 | 1 | 1 | [KHSO3] 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])^(-1) ([K2SO3])^(-1) [KOH] [KHSO3] = ([KOH] [KHSO3])/([H2O] [K2SO3])](../image_source/73db91924faadc0f76da12e9650d30ae.png)
Construct the equilibrium constant, K, expression for: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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 | 1 | -1 K_2SO_3 | 1 | -1 KOH | 1 | 1 KHSO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) K_2SO_3 | 1 | -1 | ([K2SO3])^(-1) KOH | 1 | 1 | [KOH] KHSO3 | 1 | 1 | [KHSO3] 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])^(-1) ([K2SO3])^(-1) [KOH] [KHSO3] = ([KOH] [KHSO3])/([H2O] [K2SO3])
Rate of reaction
![Construct the rate of reaction expression for: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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 | 1 | -1 K_2SO_3 | 1 | -1 KOH | 1 | 1 KHSO3 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) K_2SO_3 | 1 | -1 | -(Δ[K2SO3])/(Δt) KOH | 1 | 1 | (Δ[KOH])/(Δt) KHSO3 | 1 | 1 | (Δ[KHSO3])/(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[H2O])/(Δt) = -(Δ[K2SO3])/(Δt) = (Δ[KOH])/(Δt) = (Δ[KHSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/ebfbb19651f9fca71aebea4d0a2edf8a.png)
Construct the rate of reaction expression for: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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: H_2O + K_2SO_3 ⟶ KOH + KHSO3 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 | 1 | -1 K_2SO_3 | 1 | -1 KOH | 1 | 1 KHSO3 | 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 H_2O | 1 | -1 | -(Δ[H2O])/(Δt) K_2SO_3 | 1 | -1 | -(Δ[K2SO3])/(Δt) KOH | 1 | 1 | (Δ[KOH])/(Δt) KHSO3 | 1 | 1 | (Δ[KHSO3])/(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[H2O])/(Δt) = -(Δ[K2SO3])/(Δt) = (Δ[KOH])/(Δt) = (Δ[KHSO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| water | potassium sulfite | potassium hydroxide | KHSO3 formula | H_2O | K_2SO_3 | KOH | KHSO3 Hill formula | H_2O | K_2O_3S | HKO | HKO3S name | water | potassium sulfite | potassium hydroxide | IUPAC name | water | dipotassium sulfite | potassium hydroxide |](../image_source/1f1eb04e9d3b84684b5ca749cdd357a7.png)
| water | potassium sulfite | potassium hydroxide | KHSO3 formula | H_2O | K_2SO_3 | KOH | KHSO3 Hill formula | H_2O | K_2O_3S | HKO | HKO3S name | water | potassium sulfite | potassium hydroxide | IUPAC name | water | dipotassium sulfite | potassium hydroxide |
Substance properties
![| water | potassium sulfite | potassium hydroxide | KHSO3 molar mass | 18.015 g/mol | 158.25 g/mol | 56.105 g/mol | 120.2 g/mol phase | liquid (at STP) | | solid (at STP) | melting point | 0 °C | | 406 °C | boiling point | 99.9839 °C | | 1327 °C | density | 1 g/cm^3 | | 2.044 g/cm^3 | solubility in water | | | soluble | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 0.001 Pa s (at 550 °C) | odor | odorless | | |](../image_source/e96c9b96fdb07c279ae972f59283c7d4.png)
| water | potassium sulfite | potassium hydroxide | KHSO3 molar mass | 18.015 g/mol | 158.25 g/mol | 56.105 g/mol | 120.2 g/mol phase | liquid (at STP) | | solid (at STP) | melting point | 0 °C | | 406 °C | boiling point | 99.9839 °C | | 1327 °C | density | 1 g/cm^3 | | 2.044 g/cm^3 | solubility in water | | | soluble | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 0.001 Pa s (at 550 °C) | odor | odorless | | |
Units