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H2SO4 + H2O2 + CrO3 = H2O + O2 + Cr2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide + CrO_3 chromium trioxide ⟶ H_2O water + O_2 oxygen + Cr_2(SO_4)_3 chromium sulfate
H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide + CrO_3 chromium trioxide ⟶ H_2O water + O_2 oxygen + Cr_2(SO_4)_3 chromium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + H_2O_2 + CrO_3 ⟶ H_2O + O_2 + Cr_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2O_2 + c_3 CrO_3 ⟶ c_4 H_2O + c_5 O_2 + c_6 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 and Cr: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 2 c_2 + 3 c_3 = c_4 + 2 c_5 + 12 c_6 S: | c_1 = 3 c_6 Cr: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_2 = 1 c_3 = (2 c_1)/3 c_4 = c_1 + 1 c_5 = c_1/2 + 1/2 c_6 = c_1/3 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 3 and solve for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 2 c_4 = 4 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + H_2O_2 + 2 CrO_3 ⟶ 4 H_2O + 2 O_2 + Cr_2(SO_4)_3
Balance the chemical equation algebraically: H_2SO_4 + H_2O_2 + CrO_3 ⟶ H_2O + O_2 + Cr_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2O_2 + c_3 CrO_3 ⟶ c_4 H_2O + c_5 O_2 + c_6 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 and Cr: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 2 c_2 + 3 c_3 = c_4 + 2 c_5 + 12 c_6 S: | c_1 = 3 c_6 Cr: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_2 = 1 c_3 = (2 c_1)/3 c_4 = c_1 + 1 c_5 = c_1/2 + 1/2 c_6 = c_1/3 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 3 and solve for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 2 c_4 = 4 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + H_2O_2 + 2 CrO_3 ⟶ 4 H_2O + 2 O_2 + Cr_2(SO_4)_3

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

sulfuric acid + hydrogen peroxide + chromium trioxide ⟶ water + oxygen + chromium sulfate
sulfuric acid + hydrogen peroxide + chromium trioxide ⟶ water + oxygen + chromium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2O_2 + CrO_3 ⟶ H_2O + O_2 + 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: 3 H_2SO_4 + H_2O_2 + 2 CrO_3 ⟶ 4 H_2O + 2 O_2 + 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 | 3 | -3 H_2O_2 | 1 | -1 CrO_3 | 2 | -2 H_2O | 4 | 4 O_2 | 2 | 2 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 | 3 | -3 | ([H2SO4])^(-3) H_2O_2 | 1 | -1 | ([H2O2])^(-1) CrO_3 | 2 | -2 | ([CrO3])^(-2) H_2O | 4 | 4 | ([H2O])^4 O_2 | 2 | 2 | ([O2])^2 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])^(-3) ([H2O2])^(-1) ([CrO3])^(-2) ([H2O])^4 ([O2])^2 [Cr2(SO4)3] = (([H2O])^4 ([O2])^2 [Cr2(SO4)3])/(([H2SO4])^3 [H2O2] ([CrO3])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2O_2 + CrO_3 ⟶ H_2O + O_2 + 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: 3 H_2SO_4 + H_2O_2 + 2 CrO_3 ⟶ 4 H_2O + 2 O_2 + 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 | 3 | -3 H_2O_2 | 1 | -1 CrO_3 | 2 | -2 H_2O | 4 | 4 O_2 | 2 | 2 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 | 3 | -3 | ([H2SO4])^(-3) H_2O_2 | 1 | -1 | ([H2O2])^(-1) CrO_3 | 2 | -2 | ([CrO3])^(-2) H_2O | 4 | 4 | ([H2O])^4 O_2 | 2 | 2 | ([O2])^2 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])^(-3) ([H2O2])^(-1) ([CrO3])^(-2) ([H2O])^4 ([O2])^2 [Cr2(SO4)3] = (([H2O])^4 ([O2])^2 [Cr2(SO4)3])/(([H2SO4])^3 [H2O2] ([CrO3])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + H_2O_2 + CrO_3 ⟶ H_2O + O_2 + 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: 3 H_2SO_4 + H_2O_2 + 2 CrO_3 ⟶ 4 H_2O + 2 O_2 + 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 | 3 | -3 H_2O_2 | 1 | -1 CrO_3 | 2 | -2 H_2O | 4 | 4 O_2 | 2 | 2 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 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) CrO_3 | 2 | -2 | -1/2 (Δ[CrO3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) O_2 | 2 | 2 | 1/2 (Δ[O2])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[CrO3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/2 (Δ[O2])/(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 + H_2O_2 + CrO_3 ⟶ H_2O + O_2 + 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: 3 H_2SO_4 + H_2O_2 + 2 CrO_3 ⟶ 4 H_2O + 2 O_2 + 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 | 3 | -3 H_2O_2 | 1 | -1 CrO_3 | 2 | -2 H_2O | 4 | 4 O_2 | 2 | 2 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 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) CrO_3 | 2 | -2 | -1/2 (Δ[CrO3])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) O_2 | 2 | 2 | 1/2 (Δ[O2])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[CrO3])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/2 (Δ[O2])/(Δt) = (Δ[Cr2(SO4)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen peroxide | chromium trioxide | water | oxygen | chromium sulfate formula | H_2SO_4 | H_2O_2 | CrO_3 | H_2O | O_2 | Cr_2(SO_4)_3 Hill formula | H_2O_4S | H_2O_2 | CrO_3 | H_2O | O_2 | Cr_2O_12S_3 name | sulfuric acid | hydrogen peroxide | chromium trioxide | water | oxygen | chromium sulfate IUPAC name | sulfuric acid | hydrogen peroxide | trioxochromium | water | molecular oxygen | chromium(+3) cation trisulfate
| sulfuric acid | hydrogen peroxide | chromium trioxide | water | oxygen | chromium sulfate formula | H_2SO_4 | H_2O_2 | CrO_3 | H_2O | O_2 | Cr_2(SO_4)_3 Hill formula | H_2O_4S | H_2O_2 | CrO_3 | H_2O | O_2 | Cr_2O_12S_3 name | sulfuric acid | hydrogen peroxide | chromium trioxide | water | oxygen | chromium sulfate IUPAC name | sulfuric acid | hydrogen peroxide | trioxochromium | water | molecular oxygen | chromium(+3) cation trisulfate

Substance properties

| sulfuric acid | hydrogen peroxide | chromium trioxide | water | oxygen | chromium sulfate molar mass | 98.07 g/mol | 34.014 g/mol | 99.993 g/mol | 18.015 g/mol | 31.998 g/mol | 392.2 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | 10.371 °C | -0.43 °C | 196 °C | 0 °C | -218 °C | boiling point | 279.6 °C | 150.2 °C | | 99.9839 °C | -183 °C | 330 °C density | 1.8305 g/cm^3 | 1.44 g/cm^3 | | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 1.84 g/cm^3 solubility in water | very soluble | miscible | very soluble | | | surface tension | 0.0735 N/m | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless | odorless | odorless | odorless
| sulfuric acid | hydrogen peroxide | chromium trioxide | water | oxygen | chromium sulfate molar mass | 98.07 g/mol | 34.014 g/mol | 99.993 g/mol | 18.015 g/mol | 31.998 g/mol | 392.2 g/mol phase | liquid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | liquid (at STP) melting point | 10.371 °C | -0.43 °C | 196 °C | 0 °C | -218 °C | boiling point | 279.6 °C | 150.2 °C | | 99.9839 °C | -183 °C | 330 °C density | 1.8305 g/cm^3 | 1.44 g/cm^3 | | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 1.84 g/cm^3 solubility in water | very soluble | miscible | very soluble | | | surface tension | 0.0735 N/m | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | odorless | | odorless | odorless | odorless | odorless

Units

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