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H2SO4 + HCl + K2Cr2O7 = H2O + Cl2 + K2SO4 + Cr2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + HCl hydrogen chloride + K_2Cr_2O_7 potassium dichromate ⟶ H_2O water + Cl_2 chlorine + K_2SO_4 potassium sulfate + Cr_2(SO_4)_3 chromium sulfate
H_2SO_4 sulfuric acid + HCl hydrogen chloride + K_2Cr_2O_7 potassium dichromate ⟶ H_2O water + Cl_2 chlorine + K_2SO_4 potassium sulfate + Cr_2(SO_4)_3 chromium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + HCl + K_2Cr_2O_7 ⟶ H_2O + Cl_2 + K_2SO_4 + Cr_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HCl + c_3 K_2Cr_2O_7 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 K_2SO_4 + c_7 Cr_2(SO_4)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cl, Cr and K: H: | 2 c_1 + c_2 = 2 c_4 O: | 4 c_1 + 7 c_3 = c_4 + 4 c_6 + 12 c_7 S: | c_1 = c_6 + 3 c_7 Cl: | c_2 = 2 c_5 Cr: | 2 c_3 = 2 c_7 K: | 2 c_3 = 2 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 6 c_3 = 1 c_4 = 7 c_5 = 3 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 6 HCl + K_2Cr_2O_7 ⟶ 7 H_2O + 3 Cl_2 + K_2SO_4 + Cr_2(SO_4)_3
Balance the chemical equation algebraically: H_2SO_4 + HCl + K_2Cr_2O_7 ⟶ H_2O + Cl_2 + K_2SO_4 + Cr_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HCl + c_3 K_2Cr_2O_7 ⟶ c_4 H_2O + c_5 Cl_2 + c_6 K_2SO_4 + c_7 Cr_2(SO_4)_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cl, Cr and K: H: | 2 c_1 + c_2 = 2 c_4 O: | 4 c_1 + 7 c_3 = c_4 + 4 c_6 + 12 c_7 S: | c_1 = c_6 + 3 c_7 Cl: | c_2 = 2 c_5 Cr: | 2 c_3 = 2 c_7 K: | 2 c_3 = 2 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 6 c_3 = 1 c_4 = 7 c_5 = 3 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 6 HCl + K_2Cr_2O_7 ⟶ 7 H_2O + 3 Cl_2 + K_2SO_4 + Cr_2(SO_4)_3

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + hydrogen chloride + potassium dichromate ⟶ water + chlorine + potassium sulfate + chromium sulfate
sulfuric acid + hydrogen chloride + potassium dichromate ⟶ water + chlorine + potassium sulfate + chromium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + HCl + K_2Cr_2O_7 ⟶ H_2O + Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 + 6 HCl + K_2Cr_2O_7 ⟶ 7 H_2O + 3 Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 | 4 | -4 HCl | 6 | -6 K_2Cr_2O_7 | 1 | -1 H_2O | 7 | 7 Cl_2 | 3 | 3 K_2SO_4 | 1 | 1 Cr_2(SO_4)_3 | 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 | 4 | -4 | ([H2SO4])^(-4) HCl | 6 | -6 | ([HCl])^(-6) K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) H_2O | 7 | 7 | ([H2O])^7 Cl_2 | 3 | 3 | ([Cl2])^3 K_2SO_4 | 1 | 1 | [K2SO4] Cr_2(SO_4)_3 | 1 | 1 | [Cr2(SO4)3] 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])^(-4) ([HCl])^(-6) ([K2Cr2O7])^(-1) ([H2O])^7 ([Cl2])^3 [K2SO4] [Cr2(SO4)3] = (([H2O])^7 ([Cl2])^3 [K2SO4] [Cr2(SO4)3])/(([H2SO4])^4 ([HCl])^6 [K2Cr2O7])
Construct the equilibrium constant, K, expression for: H_2SO_4 + HCl + K_2Cr_2O_7 ⟶ H_2O + Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 + 6 HCl + K_2Cr_2O_7 ⟶ 7 H_2O + 3 Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 | 4 | -4 HCl | 6 | -6 K_2Cr_2O_7 | 1 | -1 H_2O | 7 | 7 Cl_2 | 3 | 3 K_2SO_4 | 1 | 1 Cr_2(SO_4)_3 | 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 | 4 | -4 | ([H2SO4])^(-4) HCl | 6 | -6 | ([HCl])^(-6) K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) H_2O | 7 | 7 | ([H2O])^7 Cl_2 | 3 | 3 | ([Cl2])^3 K_2SO_4 | 1 | 1 | [K2SO4] Cr_2(SO_4)_3 | 1 | 1 | [Cr2(SO4)3] 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])^(-4) ([HCl])^(-6) ([K2Cr2O7])^(-1) ([H2O])^7 ([Cl2])^3 [K2SO4] [Cr2(SO4)3] = (([H2O])^7 ([Cl2])^3 [K2SO4] [Cr2(SO4)3])/(([H2SO4])^4 ([HCl])^6 [K2Cr2O7])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + HCl + K_2Cr_2O_7 ⟶ H_2O + Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 + 6 HCl + K_2Cr_2O_7 ⟶ 7 H_2O + 3 Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 | 4 | -4 HCl | 6 | -6 K_2Cr_2O_7 | 1 | -1 H_2O | 7 | 7 Cl_2 | 3 | 3 K_2SO_4 | 1 | 1 Cr_2(SO_4)_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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) Cl_2 | 3 | 3 | 1/3 (Δ[Cl2])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Cr_2(SO_4)_3 | 1 | 1 | (Δ[Cr2(SO4)3])/(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[H2SO4])/(Δt) = -1/6 (Δ[HCl])/(Δt) = -(Δ[K2Cr2O7])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/3 (Δ[Cl2])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Cr2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + HCl + K_2Cr_2O_7 ⟶ H_2O + Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 + 6 HCl + K_2Cr_2O_7 ⟶ 7 H_2O + 3 Cl_2 + K_2SO_4 + Cr_2(SO_4)_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 H_2SO_4 | 4 | -4 HCl | 6 | -6 K_2Cr_2O_7 | 1 | -1 H_2O | 7 | 7 Cl_2 | 3 | 3 K_2SO_4 | 1 | 1 Cr_2(SO_4)_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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) HCl | 6 | -6 | -1/6 (Δ[HCl])/(Δt) K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) Cl_2 | 3 | 3 | 1/3 (Δ[Cl2])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Cr_2(SO_4)_3 | 1 | 1 | (Δ[Cr2(SO4)3])/(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[H2SO4])/(Δt) = -1/6 (Δ[HCl])/(Δt) = -(Δ[K2Cr2O7])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/3 (Δ[Cl2])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Cr2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen chloride | potassium dichromate | water | chlorine | potassium sulfate | chromium sulfate formula | H_2SO_4 | HCl | K_2Cr_2O_7 | H_2O | Cl_2 | K_2SO_4 | Cr_2(SO_4)_3 Hill formula | H_2O_4S | ClH | Cr_2K_2O_7 | H_2O | Cl_2 | K_2O_4S | Cr_2O_12S_3 name | sulfuric acid | hydrogen chloride | potassium dichromate | water | chlorine | potassium sulfate | chromium sulfate IUPAC name | sulfuric acid | hydrogen chloride | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | water | molecular chlorine | dipotassium sulfate | chromium(+3) cation trisulfate
| sulfuric acid | hydrogen chloride | potassium dichromate | water | chlorine | potassium sulfate | chromium sulfate formula | H_2SO_4 | HCl | K_2Cr_2O_7 | H_2O | Cl_2 | K_2SO_4 | Cr_2(SO_4)_3 Hill formula | H_2O_4S | ClH | Cr_2K_2O_7 | H_2O | Cl_2 | K_2O_4S | Cr_2O_12S_3 name | sulfuric acid | hydrogen chloride | potassium dichromate | water | chlorine | potassium sulfate | chromium sulfate IUPAC name | sulfuric acid | hydrogen chloride | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | water | molecular chlorine | dipotassium sulfate | chromium(+3) cation trisulfate

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