Search

H2O + Cl2 + Na2S2O3 = HCl + S + Na2SO4

Input interpretation

H_2O water + Cl_2 chlorine + Na_2S_2O_3 sodium hyposulfite ⟶ HCl hydrogen chloride + S mixed sulfur + Na_2SO_4 sodium sulfate
H_2O water + Cl_2 chlorine + Na_2S_2O_3 sodium hyposulfite ⟶ HCl hydrogen chloride + S mixed sulfur + Na_2SO_4 sodium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Na_2S_2O_3 ⟶ c_4 HCl + c_5 S + c_6 Na_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Na and S: H: | 2 c_1 = c_4 O: | c_1 + 3 c_3 = 4 c_6 Cl: | 2 c_2 = c_4 Na: | 2 c_3 = 2 c_6 S: | 2 c_3 = c_5 + c_6 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 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4
Balance the chemical equation algebraically: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cl_2 + c_3 Na_2S_2O_3 ⟶ c_4 HCl + c_5 S + c_6 Na_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cl, Na and S: H: | 2 c_1 = c_4 O: | c_1 + 3 c_3 = 4 c_6 Cl: | 2 c_2 = c_4 Na: | 2 c_3 = 2 c_6 S: | 2 c_3 = c_5 + c_6 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 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + chlorine + sodium hyposulfite ⟶ hydrogen chloride + mixed sulfur + sodium sulfate
water + chlorine + sodium hyposulfite ⟶ hydrogen chloride + mixed sulfur + sodium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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 + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 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) Cl_2 | 1 | -1 | ([Cl2])^(-1) Na_2S_2O_3 | 1 | -1 | ([Na2S2O3])^(-1) HCl | 2 | 2 | ([HCl])^2 S | 1 | 1 | [S] Na_2SO_4 | 1 | 1 | [Na2SO4] 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) ([Cl2])^(-1) ([Na2S2O3])^(-1) ([HCl])^2 [S] [Na2SO4] = (([HCl])^2 [S] [Na2SO4])/([H2O] [Cl2] [Na2S2O3])
Construct the equilibrium constant, K, expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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 + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 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) Cl_2 | 1 | -1 | ([Cl2])^(-1) Na_2S_2O_3 | 1 | -1 | ([Na2S2O3])^(-1) HCl | 2 | 2 | ([HCl])^2 S | 1 | 1 | [S] Na_2SO_4 | 1 | 1 | [Na2SO4] 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) ([Cl2])^(-1) ([Na2S2O3])^(-1) ([HCl])^2 [S] [Na2SO4] = (([HCl])^2 [S] [Na2SO4])/([H2O] [Cl2] [Na2S2O3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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 + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 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) Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) Na_2S_2O_3 | 1 | -1 | -(Δ[Na2S2O3])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(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[Cl2])/(Δt) = -(Δ[Na2S2O3])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[S])/(Δt) = (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Cl_2 + Na_2S_2O_3 ⟶ HCl + S + Na_2SO_4 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 + Cl_2 + Na_2S_2O_3 ⟶ 2 HCl + S + Na_2SO_4 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 Cl_2 | 1 | -1 Na_2S_2O_3 | 1 | -1 HCl | 2 | 2 S | 1 | 1 Na_2SO_4 | 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) Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) Na_2S_2O_3 | 1 | -1 | -(Δ[Na2S2O3])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Na_2SO_4 | 1 | 1 | (Δ[Na2SO4])/(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[Cl2])/(Δt) = -(Δ[Na2S2O3])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[S])/(Δt) = (Δ[Na2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate formula | H_2O | Cl_2 | Na_2S_2O_3 | HCl | S | Na_2SO_4 Hill formula | H_2O | Cl_2 | Na_2O_3S_2 | ClH | S | Na_2O_4S name | water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate IUPAC name | water | molecular chlorine | | hydrogen chloride | sulfur | disodium sulfate
| water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate formula | H_2O | Cl_2 | Na_2S_2O_3 | HCl | S | Na_2SO_4 Hill formula | H_2O | Cl_2 | Na_2O_3S_2 | ClH | S | Na_2O_4S name | water | chlorine | sodium hyposulfite | hydrogen chloride | mixed sulfur | sodium sulfate IUPAC name | water | molecular chlorine | | hydrogen chloride | sulfur | disodium sulfate

Random Queries

chemical types of lithium sulfate
IUPAC name of copper vs sodium fluoride
autoignition point of octane
SMILES identifier of zinc chloride
molar mass of chromium(VI) cation vs selenide anion
isotope half-lives of carbon
molar mass of pyroxene group
molar mass of triphenylphosphine hydrobromide vs tris(hydroxymethyl)phosphine
color of zinc vs bromine
CuO + H2SO3 = H2O + CuSO3