Search

Cl2 + KOH + CrI3 = H2O + KCl + K2CrO4 + KIO3

Input interpretation

Cl_2 chlorine + KOH potassium hydroxide + Cr_1I_3 chromium(III) iodide ⟶ H_2O water + KCl potassium chloride + K_2CrO_4 potassium chromate + KIO_3 potassium iodate
Cl_2 chlorine + KOH potassium hydroxide + Cr_1I_3 chromium(III) iodide ⟶ H_2O water + KCl potassium chloride + K_2CrO_4 potassium chromate + KIO_3 potassium iodate

Balanced equation

Balance the chemical equation algebraically: Cl_2 + KOH + Cr_1I_3 ⟶ H_2O + KCl + K_2CrO_4 + KIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 KOH + c_3 Cr_1I_3 ⟶ c_4 H_2O + c_5 KCl + c_6 K_2CrO_4 + c_7 KIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, O, Cr and I: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_4 K: | c_2 = c_5 + 2 c_6 + c_7 O: | c_2 = c_4 + 4 c_6 + 3 c_7 Cr: | c_3 = c_6 I: | 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 21/2 c_2 = 26 c_3 = 1 c_4 = 13 c_5 = 21 c_6 = 1 c_7 = 3 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 21 c_2 = 52 c_3 = 2 c_4 = 26 c_5 = 42 c_6 = 2 c_7 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 21 Cl_2 + 52 KOH + 2 Cr_1I_3 ⟶ 26 H_2O + 42 KCl + 2 K_2CrO_4 + 6 KIO_3
Balance the chemical equation algebraically: Cl_2 + KOH + Cr_1I_3 ⟶ H_2O + KCl + K_2CrO_4 + KIO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 KOH + c_3 Cr_1I_3 ⟶ c_4 H_2O + c_5 KCl + c_6 K_2CrO_4 + c_7 KIO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, K, O, Cr and I: Cl: | 2 c_1 = c_5 H: | c_2 = 2 c_4 K: | c_2 = c_5 + 2 c_6 + c_7 O: | c_2 = c_4 + 4 c_6 + 3 c_7 Cr: | c_3 = c_6 I: | 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 21/2 c_2 = 26 c_3 = 1 c_4 = 13 c_5 = 21 c_6 = 1 c_7 = 3 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 21 c_2 = 52 c_3 = 2 c_4 = 26 c_5 = 42 c_6 = 2 c_7 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 21 Cl_2 + 52 KOH + 2 Cr_1I_3 ⟶ 26 H_2O + 42 KCl + 2 K_2CrO_4 + 6 KIO_3

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

chlorine + potassium hydroxide + chromium(III) iodide ⟶ water + potassium chloride + potassium chromate + potassium iodate
chlorine + potassium hydroxide + chromium(III) iodide ⟶ water + potassium chloride + potassium chromate + potassium iodate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + KOH + Cr_1I_3 ⟶ H_2O + KCl + K_2CrO_4 + KIO_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: 21 Cl_2 + 52 KOH + 2 Cr_1I_3 ⟶ 26 H_2O + 42 KCl + 2 K_2CrO_4 + 6 KIO_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 Cl_2 | 21 | -21 KOH | 52 | -52 Cr_1I_3 | 2 | -2 H_2O | 26 | 26 KCl | 42 | 42 K_2CrO_4 | 2 | 2 KIO_3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 21 | -21 | ([Cl2])^(-21) KOH | 52 | -52 | ([KOH])^(-52) Cr_1I_3 | 2 | -2 | ([Cr1I3])^(-2) H_2O | 26 | 26 | ([H2O])^26 KCl | 42 | 42 | ([KCl])^42 K_2CrO_4 | 2 | 2 | ([K2CrO4])^2 KIO_3 | 6 | 6 | ([KIO3])^6 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 = ([Cl2])^(-21) ([KOH])^(-52) ([Cr1I3])^(-2) ([H2O])^26 ([KCl])^42 ([K2CrO4])^2 ([KIO3])^6 = (([H2O])^26 ([KCl])^42 ([K2CrO4])^2 ([KIO3])^6)/(([Cl2])^21 ([KOH])^52 ([Cr1I3])^2)
Construct the equilibrium constant, K, expression for: Cl_2 + KOH + Cr_1I_3 ⟶ H_2O + KCl + K_2CrO_4 + KIO_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: 21 Cl_2 + 52 KOH + 2 Cr_1I_3 ⟶ 26 H_2O + 42 KCl + 2 K_2CrO_4 + 6 KIO_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 Cl_2 | 21 | -21 KOH | 52 | -52 Cr_1I_3 | 2 | -2 H_2O | 26 | 26 KCl | 42 | 42 K_2CrO_4 | 2 | 2 KIO_3 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 21 | -21 | ([Cl2])^(-21) KOH | 52 | -52 | ([KOH])^(-52) Cr_1I_3 | 2 | -2 | ([Cr1I3])^(-2) H_2O | 26 | 26 | ([H2O])^26 KCl | 42 | 42 | ([KCl])^42 K_2CrO_4 | 2 | 2 | ([K2CrO4])^2 KIO_3 | 6 | 6 | ([KIO3])^6 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 = ([Cl2])^(-21) ([KOH])^(-52) ([Cr1I3])^(-2) ([H2O])^26 ([KCl])^42 ([K2CrO4])^2 ([KIO3])^6 = (([H2O])^26 ([KCl])^42 ([K2CrO4])^2 ([KIO3])^6)/(([Cl2])^21 ([KOH])^52 ([Cr1I3])^2)

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + KOH + Cr_1I_3 ⟶ H_2O + KCl + K_2CrO_4 + KIO_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: 21 Cl_2 + 52 KOH + 2 Cr_1I_3 ⟶ 26 H_2O + 42 KCl + 2 K_2CrO_4 + 6 KIO_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 Cl_2 | 21 | -21 KOH | 52 | -52 Cr_1I_3 | 2 | -2 H_2O | 26 | 26 KCl | 42 | 42 K_2CrO_4 | 2 | 2 KIO_3 | 6 | 6 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 Cl_2 | 21 | -21 | -1/21 (Δ[Cl2])/(Δt) KOH | 52 | -52 | -1/52 (Δ[KOH])/(Δt) Cr_1I_3 | 2 | -2 | -1/2 (Δ[Cr1I3])/(Δt) H_2O | 26 | 26 | 1/26 (Δ[H2O])/(Δt) KCl | 42 | 42 | 1/42 (Δ[KCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(Δt) KIO_3 | 6 | 6 | 1/6 (Δ[KIO3])/(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 = -1/21 (Δ[Cl2])/(Δt) = -1/52 (Δ[KOH])/(Δt) = -1/2 (Δ[Cr1I3])/(Δt) = 1/26 (Δ[H2O])/(Δt) = 1/42 (Δ[KCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) = 1/6 (Δ[KIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + KOH + Cr_1I_3 ⟶ H_2O + KCl + K_2CrO_4 + KIO_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: 21 Cl_2 + 52 KOH + 2 Cr_1I_3 ⟶ 26 H_2O + 42 KCl + 2 K_2CrO_4 + 6 KIO_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 Cl_2 | 21 | -21 KOH | 52 | -52 Cr_1I_3 | 2 | -2 H_2O | 26 | 26 KCl | 42 | 42 K_2CrO_4 | 2 | 2 KIO_3 | 6 | 6 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 Cl_2 | 21 | -21 | -1/21 (Δ[Cl2])/(Δt) KOH | 52 | -52 | -1/52 (Δ[KOH])/(Δt) Cr_1I_3 | 2 | -2 | -1/2 (Δ[Cr1I3])/(Δt) H_2O | 26 | 26 | 1/26 (Δ[H2O])/(Δt) KCl | 42 | 42 | 1/42 (Δ[KCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(Δt) KIO_3 | 6 | 6 | 1/6 (Δ[KIO3])/(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 = -1/21 (Δ[Cl2])/(Δt) = -1/52 (Δ[KOH])/(Δt) = -1/2 (Δ[Cr1I3])/(Δt) = 1/26 (Δ[H2O])/(Δt) = 1/42 (Δ[KCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) = 1/6 (Δ[KIO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | potassium hydroxide | chromium(III) iodide | water | potassium chloride | potassium chromate | potassium iodate formula | Cl_2 | KOH | Cr_1I_3 | H_2O | KCl | K_2CrO_4 | KIO_3 Hill formula | Cl_2 | HKO | CrI_3 | H_2O | ClK | CrK_2O_4 | IKO_3 name | chlorine | potassium hydroxide | chromium(III) iodide | water | potassium chloride | potassium chromate | potassium iodate IUPAC name | molecular chlorine | potassium hydroxide | triiodochromium | water | potassium chloride | dipotassium dioxido-dioxochromium | potassium iodate
| chlorine | potassium hydroxide | chromium(III) iodide | water | potassium chloride | potassium chromate | potassium iodate formula | Cl_2 | KOH | Cr_1I_3 | H_2O | KCl | K_2CrO_4 | KIO_3 Hill formula | Cl_2 | HKO | CrI_3 | H_2O | ClK | CrK_2O_4 | IKO_3 name | chlorine | potassium hydroxide | chromium(III) iodide | water | potassium chloride | potassium chromate | potassium iodate IUPAC name | molecular chlorine | potassium hydroxide | triiodochromium | water | potassium chloride | dipotassium dioxido-dioxochromium | potassium iodate

Random Queries

KOH + MnO2 + KNO3 = H2O + K2MnO4 + KNO2
density of chloroethane
crystal class of rokühnite vs kleinite
chemical uses of krypton vs 1-chloro-2,2,2-trifluoroethane
O2 + NO2 + Ca(OH)2 = H2O + Ca(NO3)2
molar mass of niobium(III) cation vs vanadium(II) cation
first ionization energy of fermium vs thorium
KOH + KClO2 + (CN)2 = H2O + KCl + N2 + K2CO3
IUPAC name of aluminum oleate
alternate names of 4-ethoxy-3,5-dimethylphenylboronic acid vs bromotrimethylsilane