Search

FeSO4 + SnSO4 = Fe2(SO4)3 + Sn

Input interpretation

FeSO_4 duretter + SnSO_4 stannous sulfate ⟶ Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + Sn white tin
FeSO_4 duretter + SnSO_4 stannous sulfate ⟶ Fe_2(SO_4)_3·xH_2O iron(III) sulfate hydrate + Sn white tin

Balanced equation

Balance the chemical equation algebraically: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO_4 + c_2 SnSO_4 ⟶ c_3 Fe_2(SO_4)_3·xH_2O + c_4 Sn Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S and Sn: Fe: | c_1 = 2 c_3 O: | 4 c_1 + 4 c_2 = 12 c_3 S: | c_1 + c_2 = 3 c_3 Sn: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn
Balance the chemical equation algebraically: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn Add stoichiometric coefficients, c_i, to the reactants and products: c_1 FeSO_4 + c_2 SnSO_4 ⟶ c_3 Fe_2(SO_4)_3·xH_2O + c_4 Sn Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, O, S and Sn: Fe: | c_1 = 2 c_3 O: | 4 c_1 + 4 c_2 = 12 c_3 S: | c_1 + c_2 = 3 c_3 Sn: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn

Structures

+ ⟶ +
+ ⟶ +

Names

duretter + stannous sulfate ⟶ iron(III) sulfate hydrate + white tin
duretter + stannous sulfate ⟶ iron(III) sulfate hydrate + white tin

Equilibrium constant

Construct the equilibrium constant, K, expression for: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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: 2 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 | 2 | -2 SnSO_4 | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Sn | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeSO_4 | 2 | -2 | ([FeSO4])^(-2) SnSO_4 | 1 | -1 | ([SnSO4])^(-1) Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] Sn | 1 | 1 | [Sn] 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 = ([FeSO4])^(-2) ([SnSO4])^(-1) [Fe2(SO4)3·xH2O] [Sn] = ([Fe2(SO4)3·xH2O] [Sn])/(([FeSO4])^2 [SnSO4])
Construct the equilibrium constant, K, expression for: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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: 2 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 | 2 | -2 SnSO_4 | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Sn | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression FeSO_4 | 2 | -2 | ([FeSO4])^(-2) SnSO_4 | 1 | -1 | ([SnSO4])^(-1) Fe_2(SO_4)_3·xH_2O | 1 | 1 | [Fe2(SO4)3·xH2O] Sn | 1 | 1 | [Sn] 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 = ([FeSO4])^(-2) ([SnSO4])^(-1) [Fe2(SO4)3·xH2O] [Sn] = ([Fe2(SO4)3·xH2O] [Sn])/(([FeSO4])^2 [SnSO4])

Rate of reaction

Construct the rate of reaction expression for: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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: 2 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 | 2 | -2 SnSO_4 | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Sn | 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 FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) SnSO_4 | 1 | -1 | -(Δ[SnSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(Δt) Sn | 1 | 1 | (Δ[Sn])/(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 = -1/2 (Δ[FeSO4])/(Δt) = -(Δ[SnSO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) = (Δ[Sn])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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: 2 FeSO_4 + SnSO_4 ⟶ Fe_2(SO_4)_3·xH_2O + Sn 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 FeSO_4 | 2 | -2 SnSO_4 | 1 | -1 Fe_2(SO_4)_3·xH_2O | 1 | 1 Sn | 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 FeSO_4 | 2 | -2 | -1/2 (Δ[FeSO4])/(Δt) SnSO_4 | 1 | -1 | -(Δ[SnSO4])/(Δt) Fe_2(SO_4)_3·xH_2O | 1 | 1 | (Δ[Fe2(SO4)3·xH2O])/(Δt) Sn | 1 | 1 | (Δ[Sn])/(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 = -1/2 (Δ[FeSO4])/(Δt) = -(Δ[SnSO4])/(Δt) = (Δ[Fe2(SO4)3·xH2O])/(Δt) = (Δ[Sn])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| duretter | stannous sulfate | iron(III) sulfate hydrate | white tin formula | FeSO_4 | SnSO_4 | Fe_2(SO_4)_3·xH_2O | Sn Hill formula | FeO_4S | O_4SSn | Fe_2O_12S_3 | Sn name | duretter | stannous sulfate | iron(III) sulfate hydrate | white tin IUPAC name | iron(+2) cation sulfate | tin(+2) cation sulfate | diferric trisulfate | tin
| duretter | stannous sulfate | iron(III) sulfate hydrate | white tin formula | FeSO_4 | SnSO_4 | Fe_2(SO_4)_3·xH_2O | Sn Hill formula | FeO_4S | O_4SSn | Fe_2O_12S_3 | Sn name | duretter | stannous sulfate | iron(III) sulfate hydrate | white tin IUPAC name | iron(+2) cation sulfate | tin(+2) cation sulfate | diferric trisulfate | tin

Substance properties

| duretter | stannous sulfate | iron(III) sulfate hydrate | white tin molar mass | 151.9 g/mol | 214.77 g/mol | 399.9 g/mol | 118.71 g/mol phase | | | | solid (at STP) melting point | | | | 231.9 °C boiling point | | | | 2602 °C density | 2.841 g/cm^3 | 4.15 g/cm^3 | | 7.31 g/cm^3 solubility in water | | soluble | slightly soluble | insoluble dynamic viscosity | | | | 0.001 Pa s (at 600 °C) odor | | | | odorless
| duretter | stannous sulfate | iron(III) sulfate hydrate | white tin molar mass | 151.9 g/mol | 214.77 g/mol | 399.9 g/mol | 118.71 g/mol phase | | | | solid (at STP) melting point | | | | 231.9 °C boiling point | | | | 2602 °C density | 2.841 g/cm^3 | 4.15 g/cm^3 | | 7.31 g/cm^3 solubility in water | | soluble | slightly soluble | insoluble dynamic viscosity | | | | 0.001 Pa s (at 600 °C) odor | | | | odorless

Units

Random Queries

boiling point of tert-butyllithium
formula of dysprosium hydride
IUPAC sodium hexafluorozirconate
invert colors kladnoite image
name of hoelite vs moolooite
iodine(I) cation vs calcium cation vs iron(II) cation
freezing point of dibromoneopentyl glycol
IUPAC name of samarium(III) phosphate hydrate vs beryl
ionic radius of hexachloroplumbate(IV) anion
bonding characteristics of californium