Search

H2SO4 + KI + NaClO = H2O + K2SO4 + I2 + NaCl

Input interpretation

H_2SO_4 sulfuric acid + KI potassium iodide + NaOCl sodium hypochlorite ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + NaCl sodium chloride
H_2SO_4 sulfuric acid + KI potassium iodide + NaOCl sodium hypochlorite ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + NaCl sodium chloride

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 NaOCl ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 NaCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K, Cl and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + c_3 = c_4 + 4 c_5 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 = 2 c_5 Cl: | c_3 = c_7 Na: | c_3 = c_7 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 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl
Balance the chemical equation algebraically: H_2SO_4 + KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KI + c_3 NaOCl ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 NaCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I, K, Cl and Na: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + c_3 = c_4 + 4 c_5 S: | c_1 = c_5 I: | c_2 = 2 c_6 K: | c_2 = 2 c_5 Cl: | c_3 = c_7 Na: | c_3 = c_7 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 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 2 KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + potassium iodide + sodium hypochlorite ⟶ water + potassium sulfate + iodine + sodium chloride
sulfuric acid + potassium iodide + sodium hypochlorite ⟶ water + potassium sulfate + iodine + sodium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 + 2 KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 | 1 | -1 KI | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 NaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) KI | 2 | -2 | ([KI])^(-2) NaOCl | 1 | -1 | ([NaOCl])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] NaCl | 1 | 1 | [NaCl] 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 = ([H2SO4])^(-1) ([KI])^(-2) ([NaOCl])^(-1) [H2O] [K2SO4] [I2] [NaCl] = ([H2O] [K2SO4] [I2] [NaCl])/([H2SO4] ([KI])^2 [NaOCl])
Construct the equilibrium constant, K, expression for: H_2SO_4 + KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 + 2 KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 | 1 | -1 KI | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 NaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) KI | 2 | -2 | ([KI])^(-2) NaOCl | 1 | -1 | ([NaOCl])^(-1) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 1 | 1 | [I2] NaCl | 1 | 1 | [NaCl] 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 = ([H2SO4])^(-1) ([KI])^(-2) ([NaOCl])^(-1) [H2O] [K2SO4] [I2] [NaCl] = ([H2O] [K2SO4] [I2] [NaCl])/([H2SO4] ([KI])^2 [NaOCl])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 + 2 KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 | 1 | -1 KI | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 NaCl | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(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[H2SO4])/(Δt) = -1/2 (Δ[KI])/(Δt) = -(Δ[NaOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[NaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 + 2 KI + NaOCl ⟶ H_2O + K_2SO_4 + I_2 + NaCl 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_2SO_4 | 1 | -1 KI | 2 | -2 NaOCl | 1 | -1 H_2O | 1 | 1 K_2SO_4 | 1 | 1 I_2 | 1 | 1 NaCl | 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) NaOCl | 1 | -1 | -(Δ[NaOCl])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(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[H2SO4])/(Δt) = -1/2 (Δ[KI])/(Δt) = -(Δ[NaOCl])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[I2])/(Δt) = (Δ[NaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium iodide | sodium hypochlorite | water | potassium sulfate | iodine | sodium chloride formula | H_2SO_4 | KI | NaOCl | H_2O | K_2SO_4 | I_2 | NaCl Hill formula | H_2O_4S | IK | ClNaO | H_2O | K_2O_4S | I_2 | ClNa name | sulfuric acid | potassium iodide | sodium hypochlorite | water | potassium sulfate | iodine | sodium chloride IUPAC name | sulfuric acid | potassium iodide | sodium hypochlorite | water | dipotassium sulfate | molecular iodine | sodium chloride
| sulfuric acid | potassium iodide | sodium hypochlorite | water | potassium sulfate | iodine | sodium chloride formula | H_2SO_4 | KI | NaOCl | H_2O | K_2SO_4 | I_2 | NaCl Hill formula | H_2O_4S | IK | ClNaO | H_2O | K_2O_4S | I_2 | ClNa name | sulfuric acid | potassium iodide | sodium hypochlorite | water | potassium sulfate | iodine | sodium chloride IUPAC name | sulfuric acid | potassium iodide | sodium hypochlorite | water | dipotassium sulfate | molecular iodine | sodium chloride

Random Queries

name of iron(III) sodium pyrophosphate vs potassium nitrite
name of lithium benzoate
tridecaborane(19) vs ammonium hexachloroosmate(IV)
CAS number of gray antimony vs scandium
edge types of tin(II) 2-ethylhexanoate vs tetramethylammonium acetate
CAS number of magnesium vs oxygen
magnetism of kadyrelite
molar mass of ammonium pentaborate tetrahydrate
tetraammineplatinum(II) nitrate vs sodium sulfate decahydrate
formula string of 10-deacetyl-2-debenzoylbaccatin iii vs cyanidin