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H2O + I2 + Cr2(SO4)3 = H2SO4 + HI + H2CrO4

Input interpretation

H_2O water + I_2 iodine + Cr_2(SO_4)_3 chromium sulfate ⟶ H_2SO_4 sulfuric acid + HI hydrogen iodide + H_2CrO_4 chromic acid
H_2O water + I_2 iodine + Cr_2(SO_4)_3 chromium sulfate ⟶ H_2SO_4 sulfuric acid + HI hydrogen iodide + H_2CrO_4 chromic acid

Balanced equation

Balance the chemical equation algebraically: H_2O + I_2 + Cr_2(SO_4)_3 ⟶ H_2SO_4 + HI + H_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I_2 + c_3 Cr_2(SO_4)_3 ⟶ c_4 H_2SO_4 + c_5 HI + c_6 H_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, I, Cr and S: H: | 2 c_1 = 2 c_4 + c_5 + 2 c_6 O: | c_1 + 12 c_3 = 4 c_4 + 4 c_6 I: | 2 c_2 = c_5 Cr: | 2 c_3 = c_6 S: | 3 c_3 = c_4 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 = 8 c_2 = 3 c_3 = 1 c_4 = 3 c_5 = 6 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2O + 3 I_2 + Cr_2(SO_4)_3 ⟶ 3 H_2SO_4 + 6 HI + 2 H_2CrO_4
Balance the chemical equation algebraically: H_2O + I_2 + Cr_2(SO_4)_3 ⟶ H_2SO_4 + HI + H_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 I_2 + c_3 Cr_2(SO_4)_3 ⟶ c_4 H_2SO_4 + c_5 HI + c_6 H_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, I, Cr and S: H: | 2 c_1 = 2 c_4 + c_5 + 2 c_6 O: | c_1 + 12 c_3 = 4 c_4 + 4 c_6 I: | 2 c_2 = c_5 Cr: | 2 c_3 = c_6 S: | 3 c_3 = c_4 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 = 8 c_2 = 3 c_3 = 1 c_4 = 3 c_5 = 6 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2O + 3 I_2 + Cr_2(SO_4)_3 ⟶ 3 H_2SO_4 + 6 HI + 2 H_2CrO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + iodine + chromium sulfate ⟶ sulfuric acid + hydrogen iodide + chromic acid
water + iodine + chromium sulfate ⟶ sulfuric acid + hydrogen iodide + chromic acid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + I_2 + Cr_2(SO_4)_3 ⟶ H_2SO_4 + HI + H_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: 8 H_2O + 3 I_2 + Cr_2(SO_4)_3 ⟶ 3 H_2SO_4 + 6 HI + 2 H_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 H_2O | 8 | -8 I_2 | 3 | -3 Cr_2(SO_4)_3 | 1 | -1 H_2SO_4 | 3 | 3 HI | 6 | 6 H_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 H_2O | 8 | -8 | ([H2O])^(-8) I_2 | 3 | -3 | ([I2])^(-3) Cr_2(SO_4)_3 | 1 | -1 | ([Cr2(SO4)3])^(-1) H_2SO_4 | 3 | 3 | ([H2SO4])^3 HI | 6 | 6 | ([HI])^6 H_2CrO_4 | 2 | 2 | ([H2CrO4])^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 = ([H2O])^(-8) ([I2])^(-3) ([Cr2(SO4)3])^(-1) ([H2SO4])^3 ([HI])^6 ([H2CrO4])^2 = (([H2SO4])^3 ([HI])^6 ([H2CrO4])^2)/(([H2O])^8 ([I2])^3 [Cr2(SO4)3])
Construct the equilibrium constant, K, expression for: H_2O + I_2 + Cr_2(SO_4)_3 ⟶ H_2SO_4 + HI + H_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: 8 H_2O + 3 I_2 + Cr_2(SO_4)_3 ⟶ 3 H_2SO_4 + 6 HI + 2 H_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 H_2O | 8 | -8 I_2 | 3 | -3 Cr_2(SO_4)_3 | 1 | -1 H_2SO_4 | 3 | 3 HI | 6 | 6 H_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 H_2O | 8 | -8 | ([H2O])^(-8) I_2 | 3 | -3 | ([I2])^(-3) Cr_2(SO_4)_3 | 1 | -1 | ([Cr2(SO4)3])^(-1) H_2SO_4 | 3 | 3 | ([H2SO4])^3 HI | 6 | 6 | ([HI])^6 H_2CrO_4 | 2 | 2 | ([H2CrO4])^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 = ([H2O])^(-8) ([I2])^(-3) ([Cr2(SO4)3])^(-1) ([H2SO4])^3 ([HI])^6 ([H2CrO4])^2 = (([H2SO4])^3 ([HI])^6 ([H2CrO4])^2)/(([H2O])^8 ([I2])^3 [Cr2(SO4)3])

Rate of reaction

Construct the rate of reaction expression for: H_2O + I_2 + Cr_2(SO_4)_3 ⟶ H_2SO_4 + HI + H_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: 8 H_2O + 3 I_2 + Cr_2(SO_4)_3 ⟶ 3 H_2SO_4 + 6 HI + 2 H_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 H_2O | 8 | -8 I_2 | 3 | -3 Cr_2(SO_4)_3 | 1 | -1 H_2SO_4 | 3 | 3 HI | 6 | 6 H_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 H_2O | 8 | -8 | -1/8 (Δ[H2O])/(Δt) I_2 | 3 | -3 | -1/3 (Δ[I2])/(Δt) Cr_2(SO_4)_3 | 1 | -1 | -(Δ[Cr2(SO4)3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) HI | 6 | 6 | 1/6 (Δ[HI])/(Δt) H_2CrO_4 | 2 | 2 | 1/2 (Δ[H2CrO4])/(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 = -1/8 (Δ[H2O])/(Δt) = -1/3 (Δ[I2])/(Δt) = -(Δ[Cr2(SO4)3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/6 (Δ[HI])/(Δt) = 1/2 (Δ[H2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + I_2 + Cr_2(SO_4)_3 ⟶ H_2SO_4 + HI + H_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: 8 H_2O + 3 I_2 + Cr_2(SO_4)_3 ⟶ 3 H_2SO_4 + 6 HI + 2 H_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 H_2O | 8 | -8 I_2 | 3 | -3 Cr_2(SO_4)_3 | 1 | -1 H_2SO_4 | 3 | 3 HI | 6 | 6 H_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 H_2O | 8 | -8 | -1/8 (Δ[H2O])/(Δt) I_2 | 3 | -3 | -1/3 (Δ[I2])/(Δt) Cr_2(SO_4)_3 | 1 | -1 | -(Δ[Cr2(SO4)3])/(Δt) H_2SO_4 | 3 | 3 | 1/3 (Δ[H2SO4])/(Δt) HI | 6 | 6 | 1/6 (Δ[HI])/(Δt) H_2CrO_4 | 2 | 2 | 1/2 (Δ[H2CrO4])/(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 = -1/8 (Δ[H2O])/(Δt) = -1/3 (Δ[I2])/(Δt) = -(Δ[Cr2(SO4)3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/6 (Δ[HI])/(Δt) = 1/2 (Δ[H2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | iodine | chromium sulfate | sulfuric acid | hydrogen iodide | chromic acid formula | H_2O | I_2 | Cr_2(SO_4)_3 | H_2SO_4 | HI | H_2CrO_4 Hill formula | H_2O | I_2 | Cr_2O_12S_3 | H_2O_4S | HI | CrH_2O_4 name | water | iodine | chromium sulfate | sulfuric acid | hydrogen iodide | chromic acid IUPAC name | water | molecular iodine | chromium(+3) cation trisulfate | sulfuric acid | hydrogen iodide | dihydroxy-dioxo-chromium
| water | iodine | chromium sulfate | sulfuric acid | hydrogen iodide | chromic acid formula | H_2O | I_2 | Cr_2(SO_4)_3 | H_2SO_4 | HI | H_2CrO_4 Hill formula | H_2O | I_2 | Cr_2O_12S_3 | H_2O_4S | HI | CrH_2O_4 name | water | iodine | chromium sulfate | sulfuric acid | hydrogen iodide | chromic acid IUPAC name | water | molecular iodine | chromium(+3) cation trisulfate | sulfuric acid | hydrogen iodide | dihydroxy-dioxo-chromium

Substance properties

| water | iodine | chromium sulfate | sulfuric acid | hydrogen iodide | chromic acid molar mass | 18.015 g/mol | 253.80894 g/mol | 392.2 g/mol | 98.07 g/mol | 127.912 g/mol | 118.01 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | 113 °C | | 10.371 °C | -50.76 °C | 196 °C boiling point | 99.9839 °C | 184 °C | 330 °C | 279.6 °C | -35.55 °C | density | 1 g/cm^3 | 4.94 g/cm^3 | 1.84 g/cm^3 | 1.8305 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 2.7 g/cm^3 solubility in water | | | | very soluble | very soluble | very soluble surface tension | 0.0728 N/m | | | 0.0735 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.00227 Pa s (at 116 °C) | | 0.021 Pa s (at 25 °C) | 0.001321 Pa s (at -39 °C) | odor | odorless | | odorless | odorless | |
| water | iodine | chromium sulfate | sulfuric acid | hydrogen iodide | chromic acid molar mass | 18.015 g/mol | 253.80894 g/mol | 392.2 g/mol | 98.07 g/mol | 127.912 g/mol | 118.01 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | 113 °C | | 10.371 °C | -50.76 °C | 196 °C boiling point | 99.9839 °C | 184 °C | 330 °C | 279.6 °C | -35.55 °C | density | 1 g/cm^3 | 4.94 g/cm^3 | 1.84 g/cm^3 | 1.8305 g/cm^3 | 0.005228 g/cm^3 (at 25 °C) | 2.7 g/cm^3 solubility in water | | | | very soluble | very soluble | very soluble surface tension | 0.0728 N/m | | | 0.0735 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.00227 Pa s (at 116 °C) | | 0.021 Pa s (at 25 °C) | 0.001321 Pa s (at -39 °C) | odor | odorless | | odorless | odorless | |

Units

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