Search

S + KOH = H2O + K2S + K2S2O3

Input interpretation

S mixed sulfur + KOH potassium hydroxide ⟶ H_2O water + K2S + K_2S_2O_3 potassium thiosulfate
S mixed sulfur + KOH potassium hydroxide ⟶ H_2O water + K2S + K_2S_2O_3 potassium thiosulfate

Balanced equation

Balance the chemical equation algebraically: S + KOH ⟶ H_2O + K2S + K_2S_2O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 S + c_2 KOH ⟶ c_3 H_2O + c_4 K2S + c_5 K_2S_2O_3 Set the number of atoms in the reactants equal to the number of atoms in the products for S, H, K and O: S: | c_1 = c_4 + 2 c_5 H: | c_2 = 2 c_3 K: | c_2 = 2 c_4 + 2 c_5 O: | c_2 = c_3 + 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 6 c_3 = 3 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 S + 6 KOH ⟶ 3 H_2O + 2 K2S + K_2S_2O_3
Balance the chemical equation algebraically: S + KOH ⟶ H_2O + K2S + K_2S_2O_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 S + c_2 KOH ⟶ c_3 H_2O + c_4 K2S + c_5 K_2S_2O_3 Set the number of atoms in the reactants equal to the number of atoms in the products for S, H, K and O: S: | c_1 = c_4 + 2 c_5 H: | c_2 = 2 c_3 K: | c_2 = 2 c_4 + 2 c_5 O: | c_2 = c_3 + 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 6 c_3 = 3 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 S + 6 KOH ⟶ 3 H_2O + 2 K2S + K_2S_2O_3

Structures

+ ⟶ + K2S +
+ ⟶ + K2S +

Names

mixed sulfur + potassium hydroxide ⟶ water + K2S + potassium thiosulfate
mixed sulfur + potassium hydroxide ⟶ water + K2S + potassium thiosulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: S + KOH ⟶ H_2O + K2S + K_2S_2O_3 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: 4 S + 6 KOH ⟶ 3 H_2O + 2 K2S + K_2S_2O_3 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 S | 4 | -4 KOH | 6 | -6 H_2O | 3 | 3 K2S | 2 | 2 K_2S_2O_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression S | 4 | -4 | ([S])^(-4) KOH | 6 | -6 | ([KOH])^(-6) H_2O | 3 | 3 | ([H2O])^3 K2S | 2 | 2 | ([K2S])^2 K_2S_2O_3 | 1 | 1 | [K2S2O3] 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 = ([S])^(-4) ([KOH])^(-6) ([H2O])^3 ([K2S])^2 [K2S2O3] = (([H2O])^3 ([K2S])^2 [K2S2O3])/(([S])^4 ([KOH])^6)
Construct the equilibrium constant, K, expression for: S + KOH ⟶ H_2O + K2S + K_2S_2O_3 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: 4 S + 6 KOH ⟶ 3 H_2O + 2 K2S + K_2S_2O_3 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 S | 4 | -4 KOH | 6 | -6 H_2O | 3 | 3 K2S | 2 | 2 K_2S_2O_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression S | 4 | -4 | ([S])^(-4) KOH | 6 | -6 | ([KOH])^(-6) H_2O | 3 | 3 | ([H2O])^3 K2S | 2 | 2 | ([K2S])^2 K_2S_2O_3 | 1 | 1 | [K2S2O3] 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 = ([S])^(-4) ([KOH])^(-6) ([H2O])^3 ([K2S])^2 [K2S2O3] = (([H2O])^3 ([K2S])^2 [K2S2O3])/(([S])^4 ([KOH])^6)

Rate of reaction

Construct the rate of reaction expression for: S + KOH ⟶ H_2O + K2S + K_2S_2O_3 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: 4 S + 6 KOH ⟶ 3 H_2O + 2 K2S + K_2S_2O_3 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 S | 4 | -4 KOH | 6 | -6 H_2O | 3 | 3 K2S | 2 | 2 K_2S_2O_3 | 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 S | 4 | -4 | -1/4 (Δ[S])/(Δt) KOH | 6 | -6 | -1/6 (Δ[KOH])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K2S | 2 | 2 | 1/2 (Δ[K2S])/(Δt) K_2S_2O_3 | 1 | 1 | (Δ[K2S2O3])/(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 = -1/4 (Δ[S])/(Δt) = -1/6 (Δ[KOH])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[K2S])/(Δt) = (Δ[K2S2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: S + KOH ⟶ H_2O + K2S + K_2S_2O_3 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: 4 S + 6 KOH ⟶ 3 H_2O + 2 K2S + K_2S_2O_3 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 S | 4 | -4 KOH | 6 | -6 H_2O | 3 | 3 K2S | 2 | 2 K_2S_2O_3 | 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 S | 4 | -4 | -1/4 (Δ[S])/(Δt) KOH | 6 | -6 | -1/6 (Δ[KOH])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K2S | 2 | 2 | 1/2 (Δ[K2S])/(Δt) K_2S_2O_3 | 1 | 1 | (Δ[K2S2O3])/(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 = -1/4 (Δ[S])/(Δt) = -1/6 (Δ[KOH])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/2 (Δ[K2S])/(Δt) = (Δ[K2S2O3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| mixed sulfur | potassium hydroxide | water | K2S | potassium thiosulfate formula | S | KOH | H_2O | K2S | K_2S_2O_3 Hill formula | S | HKO | H_2O | K2S | K_2O_3S_2 name | mixed sulfur | potassium hydroxide | water | | potassium thiosulfate IUPAC name | sulfur | potassium hydroxide | water | |
| mixed sulfur | potassium hydroxide | water | K2S | potassium thiosulfate formula | S | KOH | H_2O | K2S | K_2S_2O_3 Hill formula | S | HKO | H_2O | K2S | K_2O_3S_2 name | mixed sulfur | potassium hydroxide | water | | potassium thiosulfate IUPAC name | sulfur | potassium hydroxide | water | |

Substance properties

| mixed sulfur | potassium hydroxide | water | K2S | potassium thiosulfate molar mass | 32.06 g/mol | 56.105 g/mol | 18.015 g/mol | 110.26 g/mol | 190.3 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | | melting point | 112.8 °C | 406 °C | 0 °C | | boiling point | 444.7 °C | 1327 °C | 99.9839 °C | | density | 2.07 g/cm^3 | 2.044 g/cm^3 | 1 g/cm^3 | | 1.484 g/cm^3 solubility in water | | soluble | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | 0.001 Pa s (at 550 °C) | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |
| mixed sulfur | potassium hydroxide | water | K2S | potassium thiosulfate molar mass | 32.06 g/mol | 56.105 g/mol | 18.015 g/mol | 110.26 g/mol | 190.3 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | | melting point | 112.8 °C | 406 °C | 0 °C | | boiling point | 444.7 °C | 1327 °C | 99.9839 °C | | density | 2.07 g/cm^3 | 2.044 g/cm^3 | 1 g/cm^3 | | 1.484 g/cm^3 solubility in water | | soluble | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | 0.001 Pa s (at 550 °C) | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |

Units

Random Queries

carboxylate functional group
ion class of cobalt(III) cation vs oxide anion
hardness of nepouite crystal
CAS number of manganese(II) formate hydrate
unit cell volume of anorthite
element types of moscovium
relative molecular mass of tin allotropes
chemical types of 4-methylbenzylmagnesium chloride
InChI identifier of 3,4-di-O-acetyl-6-O-(tert-butyldimethylsilyl)-D-galactal
chemical types of tetraphenylphosphonium chloride vs gallium(III) iodide