Search

H2SO4 + K2Cr2O7 + Hg2SO4 = H2O + K2SO4 + Cr2(SO4)3 + HgSO4

Input interpretation

H_2SO_4 sulfuric acid + K_2Cr_2O_7 potassium dichromate + Hg_2SO_4 mercury(I) sulfate ⟶ H_2O water + K_2SO_4 potassium sulfate + Cr_2(SO_4)_3 chromium sulfate + HgSO_4 mercuric sulfate
H_2SO_4 sulfuric acid + K_2Cr_2O_7 potassium dichromate + Hg_2SO_4 mercury(I) sulfate ⟶ H_2O water + K_2SO_4 potassium sulfate + Cr_2(SO_4)_3 chromium sulfate + HgSO_4 mercuric sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + K_2Cr_2O_7 + Hg_2SO_4 ⟶ H_2O + K_2SO_4 + Cr_2(SO_4)_3 + HgSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 K_2Cr_2O_7 + c_3 Hg_2SO_4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 Cr_2(SO_4)_3 + c_7 HgSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cr, K and Hg: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 7 c_2 + 4 c_3 = c_4 + 4 c_5 + 12 c_6 + 4 c_7 S: | c_1 + c_3 = c_5 + 3 c_6 + c_7 Cr: | 2 c_2 = 2 c_6 K: | 2 c_2 = 2 c_5 Hg: | 2 c_3 = c_7 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 = 7 c_2 = 1 c_3 = 3 c_4 = 7 c_5 = 1 c_6 = 1 c_7 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 H_2SO_4 + K_2Cr_2O_7 + 3 Hg_2SO_4 ⟶ 7 H_2O + K_2SO_4 + Cr_2(SO_4)_3 + 6 HgSO_4
Balance the chemical equation algebraically: H_2SO_4 + K_2Cr_2O_7 + Hg_2SO_4 ⟶ H_2O + K_2SO_4 + Cr_2(SO_4)_3 + HgSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 K_2Cr_2O_7 + c_3 Hg_2SO_4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 Cr_2(SO_4)_3 + c_7 HgSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cr, K and Hg: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 7 c_2 + 4 c_3 = c_4 + 4 c_5 + 12 c_6 + 4 c_7 S: | c_1 + c_3 = c_5 + 3 c_6 + c_7 Cr: | 2 c_2 = 2 c_6 K: | 2 c_2 = 2 c_5 Hg: | 2 c_3 = c_7 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 = 7 c_2 = 1 c_3 = 3 c_4 = 7 c_5 = 1 c_6 = 1 c_7 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 H_2SO_4 + K_2Cr_2O_7 + 3 Hg_2SO_4 ⟶ 7 H_2O + K_2SO_4 + Cr_2(SO_4)_3 + 6 HgSO_4

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + potassium dichromate + mercury(I) sulfate ⟶ water + potassium sulfate + chromium sulfate + mercuric sulfate
sulfuric acid + potassium dichromate + mercury(I) sulfate ⟶ water + potassium sulfate + chromium sulfate + mercuric sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + K_2Cr_2O_7 + Hg_2SO_4 ⟶ H_2O + K_2SO_4 + Cr_2(SO_4)_3 + HgSO_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: 7 H_2SO_4 + K_2Cr_2O_7 + 3 Hg_2SO_4 ⟶ 7 H_2O + K_2SO_4 + Cr_2(SO_4)_3 + 6 HgSO_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 | 7 | -7 K_2Cr_2O_7 | 1 | -1 Hg_2SO_4 | 3 | -3 H_2O | 7 | 7 K_2SO_4 | 1 | 1 Cr_2(SO_4)_3 | 1 | 1 HgSO_4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 7 | -7 | ([H2SO4])^(-7) K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) Hg_2SO_4 | 3 | -3 | ([Hg2SO4])^(-3) H_2O | 7 | 7 | ([H2O])^7 K_2SO_4 | 1 | 1 | [K2SO4] Cr_2(SO_4)_3 | 1 | 1 | [Cr2(SO4)3] HgSO_4 | 6 | 6 | ([HgSO4])^6 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])^(-7) ([K2Cr2O7])^(-1) ([Hg2SO4])^(-3) ([H2O])^7 [K2SO4] [Cr2(SO4)3] ([HgSO4])^6 = (([H2O])^7 [K2SO4] [Cr2(SO4)3] ([HgSO4])^6)/(([H2SO4])^7 [K2Cr2O7] ([Hg2SO4])^3)
Construct the equilibrium constant, K, expression for: H_2SO_4 + K_2Cr_2O_7 + Hg_2SO_4 ⟶ H_2O + K_2SO_4 + Cr_2(SO_4)_3 + HgSO_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: 7 H_2SO_4 + K_2Cr_2O_7 + 3 Hg_2SO_4 ⟶ 7 H_2O + K_2SO_4 + Cr_2(SO_4)_3 + 6 HgSO_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 | 7 | -7 K_2Cr_2O_7 | 1 | -1 Hg_2SO_4 | 3 | -3 H_2O | 7 | 7 K_2SO_4 | 1 | 1 Cr_2(SO_4)_3 | 1 | 1 HgSO_4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 7 | -7 | ([H2SO4])^(-7) K_2Cr_2O_7 | 1 | -1 | ([K2Cr2O7])^(-1) Hg_2SO_4 | 3 | -3 | ([Hg2SO4])^(-3) H_2O | 7 | 7 | ([H2O])^7 K_2SO_4 | 1 | 1 | [K2SO4] Cr_2(SO_4)_3 | 1 | 1 | [Cr2(SO4)3] HgSO_4 | 6 | 6 | ([HgSO4])^6 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])^(-7) ([K2Cr2O7])^(-1) ([Hg2SO4])^(-3) ([H2O])^7 [K2SO4] [Cr2(SO4)3] ([HgSO4])^6 = (([H2O])^7 [K2SO4] [Cr2(SO4)3] ([HgSO4])^6)/(([H2SO4])^7 [K2Cr2O7] ([Hg2SO4])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + K_2Cr_2O_7 + Hg_2SO_4 ⟶ H_2O + K_2SO_4 + Cr_2(SO_4)_3 + HgSO_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: 7 H_2SO_4 + K_2Cr_2O_7 + 3 Hg_2SO_4 ⟶ 7 H_2O + K_2SO_4 + Cr_2(SO_4)_3 + 6 HgSO_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 | 7 | -7 K_2Cr_2O_7 | 1 | -1 Hg_2SO_4 | 3 | -3 H_2O | 7 | 7 K_2SO_4 | 1 | 1 Cr_2(SO_4)_3 | 1 | 1 HgSO_4 | 6 | 6 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 | 7 | -7 | -1/7 (Δ[H2SO4])/(Δt) K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) Hg_2SO_4 | 3 | -3 | -1/3 (Δ[Hg2SO4])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Cr_2(SO_4)_3 | 1 | 1 | (Δ[Cr2(SO4)3])/(Δt) HgSO_4 | 6 | 6 | 1/6 (Δ[HgSO4])/(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 = -1/7 (Δ[H2SO4])/(Δt) = -(Δ[K2Cr2O7])/(Δt) = -1/3 (Δ[Hg2SO4])/(Δt) = 1/7 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Cr2(SO4)3])/(Δt) = 1/6 (Δ[HgSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + K_2Cr_2O_7 + Hg_2SO_4 ⟶ H_2O + K_2SO_4 + Cr_2(SO_4)_3 + HgSO_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: 7 H_2SO_4 + K_2Cr_2O_7 + 3 Hg_2SO_4 ⟶ 7 H_2O + K_2SO_4 + Cr_2(SO_4)_3 + 6 HgSO_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 | 7 | -7 K_2Cr_2O_7 | 1 | -1 Hg_2SO_4 | 3 | -3 H_2O | 7 | 7 K_2SO_4 | 1 | 1 Cr_2(SO_4)_3 | 1 | 1 HgSO_4 | 6 | 6 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 | 7 | -7 | -1/7 (Δ[H2SO4])/(Δt) K_2Cr_2O_7 | 1 | -1 | -(Δ[K2Cr2O7])/(Δt) Hg_2SO_4 | 3 | -3 | -1/3 (Δ[Hg2SO4])/(Δt) H_2O | 7 | 7 | 1/7 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Cr_2(SO_4)_3 | 1 | 1 | (Δ[Cr2(SO4)3])/(Δt) HgSO_4 | 6 | 6 | 1/6 (Δ[HgSO4])/(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 = -1/7 (Δ[H2SO4])/(Δt) = -(Δ[K2Cr2O7])/(Δt) = -1/3 (Δ[Hg2SO4])/(Δt) = 1/7 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Cr2(SO4)3])/(Δt) = 1/6 (Δ[HgSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium dichromate | mercury(I) sulfate | water | potassium sulfate | chromium sulfate | mercuric sulfate formula | H_2SO_4 | K_2Cr_2O_7 | Hg_2SO_4 | H_2O | K_2SO_4 | Cr_2(SO_4)_3 | HgSO_4 Hill formula | H_2O_4S | Cr_2K_2O_7 | Hg_2O_4S | H_2O | K_2O_4S | Cr_2O_12S_3 | HgO_4S name | sulfuric acid | potassium dichromate | mercury(I) sulfate | water | potassium sulfate | chromium sulfate | mercuric sulfate IUPAC name | sulfuric acid | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | dimercurous sulfate | water | dipotassium sulfate | chromium(+3) cation trisulfate | mercury(+2) cation sulfate
| sulfuric acid | potassium dichromate | mercury(I) sulfate | water | potassium sulfate | chromium sulfate | mercuric sulfate formula | H_2SO_4 | K_2Cr_2O_7 | Hg_2SO_4 | H_2O | K_2SO_4 | Cr_2(SO_4)_3 | HgSO_4 Hill formula | H_2O_4S | Cr_2K_2O_7 | Hg_2O_4S | H_2O | K_2O_4S | Cr_2O_12S_3 | HgO_4S name | sulfuric acid | potassium dichromate | mercury(I) sulfate | water | potassium sulfate | chromium sulfate | mercuric sulfate IUPAC name | sulfuric acid | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | dimercurous sulfate | water | dipotassium sulfate | chromium(+3) cation trisulfate | mercury(+2) cation sulfate

Random Queries

DOT numbers of lithium peroxide vs cobalt sulfate heptahydrate
melting point of zirconium silicate
ion class of ammonium cation vs tetraethylammonium cation
formula of ammonia vs phenylmagnesium bromide
number of electrons of cesium vs calcium
Hill formula of HEPES sodium salt
PubChem CID number of iodine bromide
formula of manganese(VII) oxide vs ferrous sulfide
chemical types of sodium metasilicate vs ammonium chloropalladite
(DOT numbers of phosphorus pentachloride)/(name of phosphorus pentachloride)