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KOH + Cr2(SO4)3 + NaClO = H2O + K2SO4 + NaCl + K2CrO4

Input interpretation

KOH potassium hydroxide + Cr_2(SO_4)_3 chromium sulfate + NaOCl sodium hypochlorite ⟶ H_2O water + K_2SO_4 potassium sulfate + NaCl sodium chloride + K_2CrO_4 potassium chromate
KOH potassium hydroxide + Cr_2(SO_4)_3 chromium sulfate + NaOCl sodium hypochlorite ⟶ H_2O water + K_2SO_4 potassium sulfate + NaCl sodium chloride + K_2CrO_4 potassium chromate

Balanced equation

Balance the chemical equation algebraically: KOH + Cr_2(SO_4)_3 + NaOCl ⟶ H_2O + K_2SO_4 + NaCl + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 Cr_2(SO_4)_3 + c_3 NaOCl ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 NaCl + c_7 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Cr, S, Cl and Na: H: | c_1 = 2 c_4 K: | c_1 = 2 c_5 + 2 c_7 O: | c_1 + 12 c_2 + c_3 = c_4 + 4 c_5 + 4 c_7 Cr: | 2 c_2 = c_7 S: | 3 c_2 = c_5 Cl: | c_3 = c_6 Na: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 1 c_3 = 3 c_4 = 5 c_5 = 3 c_6 = 3 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 KOH + Cr_2(SO_4)_3 + 3 NaOCl ⟶ 5 H_2O + 3 K_2SO_4 + 3 NaCl + 2 K_2CrO_4
Balance the chemical equation algebraically: KOH + Cr_2(SO_4)_3 + NaOCl ⟶ H_2O + K_2SO_4 + NaCl + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 Cr_2(SO_4)_3 + c_3 NaOCl ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 NaCl + c_7 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Cr, S, Cl and Na: H: | c_1 = 2 c_4 K: | c_1 = 2 c_5 + 2 c_7 O: | c_1 + 12 c_2 + c_3 = c_4 + 4 c_5 + 4 c_7 Cr: | 2 c_2 = c_7 S: | 3 c_2 = c_5 Cl: | c_3 = c_6 Na: | c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 1 c_3 = 3 c_4 = 5 c_5 = 3 c_6 = 3 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 KOH + Cr_2(SO_4)_3 + 3 NaOCl ⟶ 5 H_2O + 3 K_2SO_4 + 3 NaCl + 2 K_2CrO_4

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

potassium hydroxide + chromium sulfate + sodium hypochlorite ⟶ water + potassium sulfate + sodium chloride + potassium chromate
potassium hydroxide + chromium sulfate + sodium hypochlorite ⟶ water + potassium sulfate + sodium chloride + potassium chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + Cr_2(SO_4)_3 + NaOCl ⟶ H_2O + K_2SO_4 + NaCl + K_2CrO_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: 10 KOH + Cr_2(SO_4)_3 + 3 NaOCl ⟶ 5 H_2O + 3 K_2SO_4 + 3 NaCl + 2 K_2CrO_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 KOH | 10 | -10 Cr_2(SO_4)_3 | 1 | -1 NaOCl | 3 | -3 H_2O | 5 | 5 K_2SO_4 | 3 | 3 NaCl | 3 | 3 K_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 10 | -10 | ([KOH])^(-10) Cr_2(SO_4)_3 | 1 | -1 | ([Cr2(SO4)3])^(-1) NaOCl | 3 | -3 | ([NaOCl])^(-3) H_2O | 5 | 5 | ([H2O])^5 K_2SO_4 | 3 | 3 | ([K2SO4])^3 NaCl | 3 | 3 | ([NaCl])^3 K_2CrO_4 | 2 | 2 | ([K2CrO4])^2 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 = ([KOH])^(-10) ([Cr2(SO4)3])^(-1) ([NaOCl])^(-3) ([H2O])^5 ([K2SO4])^3 ([NaCl])^3 ([K2CrO4])^2 = (([H2O])^5 ([K2SO4])^3 ([NaCl])^3 ([K2CrO4])^2)/(([KOH])^10 [Cr2(SO4)3] ([NaOCl])^3)
Construct the equilibrium constant, K, expression for: KOH + Cr_2(SO_4)_3 + NaOCl ⟶ H_2O + K_2SO_4 + NaCl + K_2CrO_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: 10 KOH + Cr_2(SO_4)_3 + 3 NaOCl ⟶ 5 H_2O + 3 K_2SO_4 + 3 NaCl + 2 K_2CrO_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 KOH | 10 | -10 Cr_2(SO_4)_3 | 1 | -1 NaOCl | 3 | -3 H_2O | 5 | 5 K_2SO_4 | 3 | 3 NaCl | 3 | 3 K_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 10 | -10 | ([KOH])^(-10) Cr_2(SO_4)_3 | 1 | -1 | ([Cr2(SO4)3])^(-1) NaOCl | 3 | -3 | ([NaOCl])^(-3) H_2O | 5 | 5 | ([H2O])^5 K_2SO_4 | 3 | 3 | ([K2SO4])^3 NaCl | 3 | 3 | ([NaCl])^3 K_2CrO_4 | 2 | 2 | ([K2CrO4])^2 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 = ([KOH])^(-10) ([Cr2(SO4)3])^(-1) ([NaOCl])^(-3) ([H2O])^5 ([K2SO4])^3 ([NaCl])^3 ([K2CrO4])^2 = (([H2O])^5 ([K2SO4])^3 ([NaCl])^3 ([K2CrO4])^2)/(([KOH])^10 [Cr2(SO4)3] ([NaOCl])^3)

Rate of reaction

Construct the rate of reaction expression for: KOH + Cr_2(SO_4)_3 + NaOCl ⟶ H_2O + K_2SO_4 + NaCl + K_2CrO_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: 10 KOH + Cr_2(SO_4)_3 + 3 NaOCl ⟶ 5 H_2O + 3 K_2SO_4 + 3 NaCl + 2 K_2CrO_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 KOH | 10 | -10 Cr_2(SO_4)_3 | 1 | -1 NaOCl | 3 | -3 H_2O | 5 | 5 K_2SO_4 | 3 | 3 NaCl | 3 | 3 K_2CrO_4 | 2 | 2 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 KOH | 10 | -10 | -1/10 (Δ[KOH])/(Δt) Cr_2(SO_4)_3 | 1 | -1 | -(Δ[Cr2(SO4)3])/(Δt) NaOCl | 3 | -3 | -1/3 (Δ[NaOCl])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) NaCl | 3 | 3 | 1/3 (Δ[NaCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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 = -1/10 (Δ[KOH])/(Δt) = -(Δ[Cr2(SO4)3])/(Δt) = -1/3 (Δ[NaOCl])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/3 (Δ[NaCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + Cr_2(SO_4)_3 + NaOCl ⟶ H_2O + K_2SO_4 + NaCl + K_2CrO_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: 10 KOH + Cr_2(SO_4)_3 + 3 NaOCl ⟶ 5 H_2O + 3 K_2SO_4 + 3 NaCl + 2 K_2CrO_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 KOH | 10 | -10 Cr_2(SO_4)_3 | 1 | -1 NaOCl | 3 | -3 H_2O | 5 | 5 K_2SO_4 | 3 | 3 NaCl | 3 | 3 K_2CrO_4 | 2 | 2 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 KOH | 10 | -10 | -1/10 (Δ[KOH])/(Δt) Cr_2(SO_4)_3 | 1 | -1 | -(Δ[Cr2(SO4)3])/(Δt) NaOCl | 3 | -3 | -1/3 (Δ[NaOCl])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) NaCl | 3 | 3 | 1/3 (Δ[NaCl])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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 = -1/10 (Δ[KOH])/(Δt) = -(Δ[Cr2(SO4)3])/(Δt) = -1/3 (Δ[NaOCl])/(Δt) = 1/5 (Δ[H2O])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/3 (Δ[NaCl])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | chromium sulfate | sodium hypochlorite | water | potassium sulfate | sodium chloride | potassium chromate formula | KOH | Cr_2(SO_4)_3 | NaOCl | H_2O | K_2SO_4 | NaCl | K_2CrO_4 Hill formula | HKO | Cr_2O_12S_3 | ClNaO | H_2O | K_2O_4S | ClNa | CrK_2O_4 name | potassium hydroxide | chromium sulfate | sodium hypochlorite | water | potassium sulfate | sodium chloride | potassium chromate IUPAC name | potassium hydroxide | chromium(+3) cation trisulfate | sodium hypochlorite | water | dipotassium sulfate | sodium chloride | dipotassium dioxido-dioxochromium
| potassium hydroxide | chromium sulfate | sodium hypochlorite | water | potassium sulfate | sodium chloride | potassium chromate formula | KOH | Cr_2(SO_4)_3 | NaOCl | H_2O | K_2SO_4 | NaCl | K_2CrO_4 Hill formula | HKO | Cr_2O_12S_3 | ClNaO | H_2O | K_2O_4S | ClNa | CrK_2O_4 name | potassium hydroxide | chromium sulfate | sodium hypochlorite | water | potassium sulfate | sodium chloride | potassium chromate IUPAC name | potassium hydroxide | chromium(+3) cation trisulfate | sodium hypochlorite | water | dipotassium sulfate | sodium chloride | dipotassium dioxido-dioxochromium

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