H2SO4 + H2S + K2Cr2O7 = H2O + S + Cr2(SO4)3 + K2O4

H_2SO_4 sulfuric acid + H_2S hydrogen sulfide + K_2Cr_2O_7 potassium dichromate ⟶ H_2O water + S mixed sulfur + Cr_2(SO_4)_3 chromium sulfate + K2O4

Balance the chemical equation algebraically: H_2SO_4 + H_2S + K_2Cr_2O_7 ⟶ H_2O + S + Cr_2(SO_4)_3 + K2O4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2S + c_3 K_2Cr_2O_7 ⟶ c_4 H_2O + c_5 S + c_6 Cr_2(SO_4)_3 + c_7 K2O4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cr and K: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 7 c_3 = c_4 + 12 c_6 + 4 c_7 S: | c_1 + c_2 = c_5 + 3 c_6 Cr: | 2 c_3 = 2 c_6 K: | 2 c_3 = 2 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_2 = 3 c_1 - 9 c_3 = 1 c_4 = 4 c_1 - 9 c_5 = 4 c_1 - 12 c_6 = 1 c_7 = 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 4 and solve for the remaining coefficients: c_1 = 4 c_2 = 3 c_3 = 1 c_4 = 7 c_5 = 4 c_6 = 1 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 3 H_2S + K_2Cr_2O_7 ⟶ 7 H_2O + 4 S + Cr_2(SO_4)_3 + K2O4

+ + ⟶ + + + K2O4

sulfuric acid + hydrogen sulfide + potassium dichromate ⟶ water + mixed sulfur + chromium sulfate + K2O4

Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2S + K_2Cr_2O_7 ⟶ H_2O + S + Cr_2(SO_4)_3 + K2O4 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 + 3 H_2S + K_2Cr_2O_7 ⟶ 7 H_2O + 4 S + Cr_2(SO_4)_3 + K2O4 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 H_2S | 3 | -3 K_2Cr_2O_7 | 1 | -1 H_2O | 7 | 7 S | 4 | 4 Cr_2(SO_4)_3 | 1 | 1 K2O4 | 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) H_2S | 3 | -3 | ([H2S])^(-3) K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) H_2O | 7 | 7 | ([H2O])^7 S | 4 | 4 | ([S])^4 Cr_2(SO_4)_3 | 1 | 1 | [Cr2(SO4)3] K2O4 | 1 | 1 | [K2O4] 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) ([H2S])^(-3) ([K2Cr2O7])^(-1) ([H2O])^7 ([S])^4 [Cr2(SO4)3] [K2O4] = (([H2O])^7 ([S])^4 [Cr2(SO4)3] [K2O4])/(([H2SO4])^4 ([H2S])^3 [K2Cr2O7])

Construct the rate of reaction expression for: H_2SO_4 + H_2S + K_2Cr_2O_7 ⟶ H_2O + S + Cr_2(SO_4)_3 + K2O4 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 + 3 H_2S + K_2Cr_2O_7 ⟶ 7 H_2O + 4 S + Cr_2(SO_4)_3 + K2O4 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 H_2S | 3 | -3 K_2Cr_2O_7 | 1 | -1 H_2O | 7 | 7 S | 4 | 4 Cr_2(SO_4)_3 | 1 | 1 K2O4 | 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) H_2S | 3 | -3 | -1/3 (Δ[H2S])/(Δt) K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) S | 4 | 4 | 1/4 (Δ[S])/(Δt) Cr_2(SO_4)_3 | 1 | 1 | (Δ[Cr2(SO4)3])/(Δt) K2O4 | 1 | 1 | (Δ[K2O4])/(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) = -1/3 (Δ[H2S])/(Δt) = -(Δ[K2Cr2O7])/(Δt) = 1/7 (Δ[H2O])/(Δt) = 1/4 (Δ[S])/(Δt) = (Δ[Cr2(SO4)3])/(Δt) = (Δ[K2O4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | hydrogen sulfide | potassium dichromate | water | mixed sulfur | chromium sulfate | K2O4 formula | H_2SO_4 | H_2S | K_2Cr_2O_7 | H_2O | S | Cr_2(SO_4)_3 | K2O4 Hill formula | H_2O_4S | H_2S | Cr_2K_2O_7 | H_2O | S | Cr_2O_12S_3 | K2O4 name | sulfuric acid | hydrogen sulfide | potassium dichromate | water | mixed sulfur | chromium sulfate | IUPAC name | sulfuric acid | hydrogen sulfide | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | water | sulfur | chromium(+3) cation trisulfate |

| sulfuric acid | hydrogen sulfide | potassium dichromate | water | mixed sulfur | chromium sulfate | K2O4 molar mass | 98.07 g/mol | 34.08 g/mol | 294.18 g/mol | 18.015 g/mol | 32.06 g/mol | 392.2 g/mol | 142.19 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | melting point | 10.371 °C | -85 °C | 398 °C | 0 °C | 112.8 °C | | boiling point | 279.6 °C | -60 °C | | 99.9839 °C | 444.7 °C | 330 °C | density | 1.8305 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 2.67 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 | 1.84 g/cm^3 | solubility in water | very soluble | | | | | | surface tension | 0.0735 N/m | | | 0.0728 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | 1.239×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | | odor | odorless | | odorless | odorless | | odorless |