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H2SO4 + Cr = H2O + S + Cr2(SO4)3

Input interpretation

H_2SO_4 sulfuric acid + Cr chromium ⟶ H_2O water + S mixed sulfur + Cr_2(SO_4)_3 chromium sulfate
H_2SO_4 sulfuric acid + Cr chromium ⟶ H_2O water + S mixed sulfur + Cr_2(SO_4)_3 chromium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + Cr ⟶ H_2O + S + Cr_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Cr ⟶ c_3 H_2O + c_4 S + c_5 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_3 O: | 4 c_1 = c_3 + 12 c_5 S: | c_1 = c_4 + 3 c_5 Cr: | c_2 = 2 c_5 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 2 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 2 Cr ⟶ 4 H_2O + S + Cr_2(SO_4)_3
Balance the chemical equation algebraically: H_2SO_4 + Cr ⟶ H_2O + S + Cr_2(SO_4)_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Cr ⟶ c_3 H_2O + c_4 S + c_5 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_3 O: | 4 c_1 = c_3 + 12 c_5 S: | c_1 = c_4 + 3 c_5 Cr: | c_2 = 2 c_5 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 2 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 2 Cr ⟶ 4 H_2O + S + Cr_2(SO_4)_3

Structures

+ ⟶ + +
+ ⟶ + +

Names

sulfuric acid + chromium ⟶ water + mixed sulfur + chromium sulfate
sulfuric acid + chromium ⟶ water + mixed sulfur + chromium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + Cr ⟶ H_2O + S + 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 + 2 Cr ⟶ 4 H_2O + S + 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 Cr | 2 | -2 H_2O | 4 | 4 S | 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) Cr | 2 | -2 | ([Cr])^(-2) H_2O | 4 | 4 | ([H2O])^4 S | 1 | 1 | [S] 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) ([Cr])^(-2) ([H2O])^4 [S] [Cr2(SO4)3] = (([H2O])^4 [S] [Cr2(SO4)3])/(([H2SO4])^4 ([Cr])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + Cr ⟶ H_2O + S + 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 + 2 Cr ⟶ 4 H_2O + S + 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 Cr | 2 | -2 H_2O | 4 | 4 S | 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) Cr | 2 | -2 | ([Cr])^(-2) H_2O | 4 | 4 | ([H2O])^4 S | 1 | 1 | [S] 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) ([Cr])^(-2) ([H2O])^4 [S] [Cr2(SO4)3] = (([H2O])^4 [S] [Cr2(SO4)3])/(([H2SO4])^4 ([Cr])^2)

Rate of reaction

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

Chemical names and formulas

| sulfuric acid | chromium | water | mixed sulfur | chromium sulfate formula | H_2SO_4 | Cr | H_2O | S | Cr_2(SO_4)_3 Hill formula | H_2O_4S | Cr | H_2O | S | Cr_2O_12S_3 name | sulfuric acid | chromium | water | mixed sulfur | chromium sulfate IUPAC name | sulfuric acid | chromium | water | sulfur | chromium(+3) cation trisulfate
| sulfuric acid | chromium | water | mixed sulfur | chromium sulfate formula | H_2SO_4 | Cr | H_2O | S | Cr_2(SO_4)_3 Hill formula | H_2O_4S | Cr | H_2O | S | Cr_2O_12S_3 name | sulfuric acid | chromium | water | mixed sulfur | chromium sulfate IUPAC name | sulfuric acid | chromium | water | sulfur | chromium(+3) cation trisulfate

Substance properties

| sulfuric acid | chromium | water | mixed sulfur | chromium sulfate molar mass | 98.07 g/mol | 51.9961 g/mol | 18.015 g/mol | 32.06 g/mol | 392.2 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) melting point | 10.371 °C | 1857 °C | 0 °C | 112.8 °C | boiling point | 279.6 °C | 2672 °C | 99.9839 °C | 444.7 °C | 330 °C density | 1.8305 g/cm^3 | 7.14 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 | 1.84 g/cm^3 solubility in water | very soluble | insoluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | odorless | odorless | | odorless
| sulfuric acid | chromium | water | mixed sulfur | chromium sulfate molar mass | 98.07 g/mol | 51.9961 g/mol | 18.015 g/mol | 32.06 g/mol | 392.2 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) melting point | 10.371 °C | 1857 °C | 0 °C | 112.8 °C | boiling point | 279.6 °C | 2672 °C | 99.9839 °C | 444.7 °C | 330 °C density | 1.8305 g/cm^3 | 7.14 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 | 1.84 g/cm^3 solubility in water | very soluble | insoluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | odorless | odorless | | odorless

Units

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