Search

H2SO4 + (FeOH)2SO4 = H2O + FeSO4

Input interpretation

H_2SO_4 sulfuric acid + (FeOH)2SO4 ⟶ H_2O water + FeSO_4 duretter
H_2SO_4 sulfuric acid + (FeOH)2SO4 ⟶ H_2O water + FeSO_4 duretter

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + (FeOH)2SO4 ⟶ H_2O + FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 (FeOH)2SO4 ⟶ c_3 H_2O + c_4 FeSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Fe: H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 4 c_1 + 6 c_2 = c_3 + 4 c_4 S: | c_1 + c_2 = c_4 Fe: | 2 c_2 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + (FeOH)2SO4 ⟶ 2 H_2O + 2 FeSO_4
Balance the chemical equation algebraically: H_2SO_4 + (FeOH)2SO4 ⟶ H_2O + FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 (FeOH)2SO4 ⟶ c_3 H_2O + c_4 FeSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Fe: H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 4 c_1 + 6 c_2 = c_3 + 4 c_4 S: | c_1 + c_2 = c_4 Fe: | 2 c_2 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + (FeOH)2SO4 ⟶ 2 H_2O + 2 FeSO_4

Structures

+ (FeOH)2SO4 ⟶ +
+ (FeOH)2SO4 ⟶ +

Names

sulfuric acid + (FeOH)2SO4 ⟶ water + duretter
sulfuric acid + (FeOH)2SO4 ⟶ water + duretter

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + (FeOH)2SO4 ⟶ H_2O + FeSO_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: H_2SO_4 + (FeOH)2SO4 ⟶ 2 H_2O + 2 FeSO_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_2SO_4 | 1 | -1 (FeOH)2SO4 | 1 | -1 H_2O | 2 | 2 FeSO_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_2SO_4 | 1 | -1 | ([H2SO4])^(-1) (FeOH)2SO4 | 1 | -1 | ([(FeOH)2SO4])^(-1) H_2O | 2 | 2 | ([H2O])^2 FeSO_4 | 2 | 2 | ([FeSO4])^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 = ([H2SO4])^(-1) ([(FeOH)2SO4])^(-1) ([H2O])^2 ([FeSO4])^2 = (([H2O])^2 ([FeSO4])^2)/([H2SO4] [(FeOH)2SO4])
Construct the equilibrium constant, K, expression for: H_2SO_4 + (FeOH)2SO4 ⟶ H_2O + FeSO_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: H_2SO_4 + (FeOH)2SO4 ⟶ 2 H_2O + 2 FeSO_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_2SO_4 | 1 | -1 (FeOH)2SO4 | 1 | -1 H_2O | 2 | 2 FeSO_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_2SO_4 | 1 | -1 | ([H2SO4])^(-1) (FeOH)2SO4 | 1 | -1 | ([(FeOH)2SO4])^(-1) H_2O | 2 | 2 | ([H2O])^2 FeSO_4 | 2 | 2 | ([FeSO4])^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 = ([H2SO4])^(-1) ([(FeOH)2SO4])^(-1) ([H2O])^2 ([FeSO4])^2 = (([H2O])^2 ([FeSO4])^2)/([H2SO4] [(FeOH)2SO4])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + (FeOH)2SO4 ⟶ H_2O + FeSO_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: H_2SO_4 + (FeOH)2SO4 ⟶ 2 H_2O + 2 FeSO_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_2SO_4 | 1 | -1 (FeOH)2SO4 | 1 | -1 H_2O | 2 | 2 FeSO_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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) (FeOH)2SO4 | 1 | -1 | -(Δ[(FeOH)2SO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) FeSO_4 | 2 | 2 | 1/2 (Δ[FeSO4])/(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 = -(Δ[H2SO4])/(Δt) = -(Δ[(FeOH)2SO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + (FeOH)2SO4 ⟶ H_2O + FeSO_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: H_2SO_4 + (FeOH)2SO4 ⟶ 2 H_2O + 2 FeSO_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_2SO_4 | 1 | -1 (FeOH)2SO4 | 1 | -1 H_2O | 2 | 2 FeSO_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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) (FeOH)2SO4 | 1 | -1 | -(Δ[(FeOH)2SO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) FeSO_4 | 2 | 2 | 1/2 (Δ[FeSO4])/(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 = -(Δ[H2SO4])/(Δt) = -(Δ[(FeOH)2SO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | (FeOH)2SO4 | water | duretter formula | H_2SO_4 | (FeOH)2SO4 | H_2O | FeSO_4 Hill formula | H_2O_4S | H2Fe2O6S | H_2O | FeO_4S name | sulfuric acid | | water | duretter IUPAC name | sulfuric acid | | water | iron(+2) cation sulfate
| sulfuric acid | (FeOH)2SO4 | water | duretter formula | H_2SO_4 | (FeOH)2SO4 | H_2O | FeSO_4 Hill formula | H_2O_4S | H2Fe2O6S | H_2O | FeO_4S name | sulfuric acid | | water | duretter IUPAC name | sulfuric acid | | water | iron(+2) cation sulfate

Substance properties

| sulfuric acid | (FeOH)2SO4 | water | duretter molar mass | 98.07 g/mol | 241.76 g/mol | 18.015 g/mol | 151.9 g/mol phase | liquid (at STP) | | liquid (at STP) | melting point | 10.371 °C | | 0 °C | boiling point | 279.6 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | | 1 g/cm^3 | 2.841 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) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |
| sulfuric acid | (FeOH)2SO4 | water | duretter molar mass | 98.07 g/mol | 241.76 g/mol | 18.015 g/mol | 151.9 g/mol phase | liquid (at STP) | | liquid (at STP) | melting point | 10.371 °C | | 0 °C | boiling point | 279.6 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | | 1 g/cm^3 | 2.841 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) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |

Units

Random Queries

structure diagram of oxygen(I) cation vs aluminum cation
diethylamine
freezing point of sodium nitrate vs lithium hydroxide
HNO3 + Al = H2O + N2 + N2O + Al(NO3)3
element types of acetic acid vs 1-butanol
alternate names of chromium trioxide
IUPAC name of potassium hydrogen tartrate
CAS (Z)-2-(chloroacetamido)-alpha-(methoxyimino)thiazol-4-acetic acid
IUPAC name of N-(tert-butoxycarbonyl)-D-prolinal vs 4-fluoroaniline
ion class of nitride anion vs acetate anion