Search

H2SO4 + K2Cr2O7 + P2S5 = H2O + K2SO4 + SO2 + Cr2(SO4)3 + K3PO4

Input interpretation

H_2SO_4 sulfuric acid + K_2Cr_2O_7 potassium dichromate + P_2S_5 phosphorus pentasulfide ⟶ H_2O water + K_2SO_4 potassium sulfate + SO_2 sulfur dioxide + Cr_2(SO_4)_3 chromium sulfate + K3PO4
H_2SO_4 sulfuric acid + K_2Cr_2O_7 potassium dichromate + P_2S_5 phosphorus pentasulfide ⟶ H_2O water + K_2SO_4 potassium sulfate + SO_2 sulfur dioxide + Cr_2(SO_4)_3 chromium sulfate + K3PO4

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + K_2Cr_2O_7 + P_2S_5 ⟶ H_2O + K_2SO_4 + SO_2 + Cr_2(SO_4)_3 + K3PO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 K_2Cr_2O_7 + c_3 P_2S_5 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 SO_2 + c_7 Cr_2(SO_4)_3 + c_8 K3PO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cr, K and P: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 7 c_2 = c_4 + 4 c_5 + 2 c_6 + 12 c_7 + 4 c_8 S: | c_1 + 5 c_3 = c_5 + c_6 + 3 c_7 Cr: | 2 c_2 = 2 c_7 K: | 2 c_2 = 2 c_5 + 3 c_8 P: | 2 c_3 = c_8 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1 - 12 c_3 = 1 c_4 = c_1 c_5 = c_1 - 15 c_6 = 56 - 3 c_1 c_7 = c_1 - 12 c_8 = 2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 16 and solve for the remaining coefficients: c_1 = 16 c_2 = 4 c_3 = 1 c_4 = 16 c_5 = 1 c_6 = 8 c_7 = 4 c_8 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 16 H_2SO_4 + 4 K_2Cr_2O_7 + P_2S_5 ⟶ 16 H_2O + K_2SO_4 + 8 SO_2 + 4 Cr_2(SO_4)_3 + 2 K3PO4
Balance the chemical equation algebraically: H_2SO_4 + K_2Cr_2O_7 + P_2S_5 ⟶ H_2O + K_2SO_4 + SO_2 + Cr_2(SO_4)_3 + K3PO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 K_2Cr_2O_7 + c_3 P_2S_5 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 SO_2 + c_7 Cr_2(SO_4)_3 + c_8 K3PO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cr, K and P: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 7 c_2 = c_4 + 4 c_5 + 2 c_6 + 12 c_7 + 4 c_8 S: | c_1 + 5 c_3 = c_5 + c_6 + 3 c_7 Cr: | 2 c_2 = 2 c_7 K: | 2 c_2 = 2 c_5 + 3 c_8 P: | 2 c_3 = c_8 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1 - 12 c_3 = 1 c_4 = c_1 c_5 = c_1 - 15 c_6 = 56 - 3 c_1 c_7 = c_1 - 12 c_8 = 2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 16 and solve for the remaining coefficients: c_1 = 16 c_2 = 4 c_3 = 1 c_4 = 16 c_5 = 1 c_6 = 8 c_7 = 4 c_8 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 16 H_2SO_4 + 4 K_2Cr_2O_7 + P_2S_5 ⟶ 16 H_2O + K_2SO_4 + 8 SO_2 + 4 Cr_2(SO_4)_3 + 2 K3PO4

Structures

+ + ⟶ + + + + K3PO4
+ + ⟶ + + + + K3PO4

Names

sulfuric acid + potassium dichromate + phosphorus pentasulfide ⟶ water + potassium sulfate + sulfur dioxide + chromium sulfate + K3PO4
sulfuric acid + potassium dichromate + phosphorus pentasulfide ⟶ water + potassium sulfate + sulfur dioxide + chromium sulfate + K3PO4

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + K_2Cr_2O_7 + P_2S_5 ⟶ H_2O + K_2SO_4 + SO_2 + Cr_2(SO_4)_3 + K3PO4 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: 16 H_2SO_4 + 4 K_2Cr_2O_7 + P_2S_5 ⟶ 16 H_2O + K_2SO_4 + 8 SO_2 + 4 Cr_2(SO_4)_3 + 2 K3PO4 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 | 16 | -16 K_2Cr_2O_7 | 4 | -4 P_2S_5 | 1 | -1 H_2O | 16 | 16 K_2SO_4 | 1 | 1 SO_2 | 8 | 8 Cr_2(SO_4)_3 | 4 | 4 K3PO4 | 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 | 16 | -16 | ([H2SO4])^(-16) K_2Cr_2O_7 | 4 | -4 | ([K2Cr2O7])^(-4) P_2S_5 | 1 | -1 | ([P2S5])^(-1) H_2O | 16 | 16 | ([H2O])^16 K_2SO_4 | 1 | 1 | [K2SO4] SO_2 | 8 | 8 | ([SO2])^8 Cr_2(SO_4)_3 | 4 | 4 | ([Cr2(SO4)3])^4 K3PO4 | 2 | 2 | ([K3PO4])^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])^(-16) ([K2Cr2O7])^(-4) ([P2S5])^(-1) ([H2O])^16 [K2SO4] ([SO2])^8 ([Cr2(SO4)3])^4 ([K3PO4])^2 = (([H2O])^16 [K2SO4] ([SO2])^8 ([Cr2(SO4)3])^4 ([K3PO4])^2)/(([H2SO4])^16 ([K2Cr2O7])^4 [P2S5])
Construct the equilibrium constant, K, expression for: H_2SO_4 + K_2Cr_2O_7 + P_2S_5 ⟶ H_2O + K_2SO_4 + SO_2 + Cr_2(SO_4)_3 + K3PO4 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: 16 H_2SO_4 + 4 K_2Cr_2O_7 + P_2S_5 ⟶ 16 H_2O + K_2SO_4 + 8 SO_2 + 4 Cr_2(SO_4)_3 + 2 K3PO4 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 | 16 | -16 K_2Cr_2O_7 | 4 | -4 P_2S_5 | 1 | -1 H_2O | 16 | 16 K_2SO_4 | 1 | 1 SO_2 | 8 | 8 Cr_2(SO_4)_3 | 4 | 4 K3PO4 | 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 | 16 | -16 | ([H2SO4])^(-16) K_2Cr_2O_7 | 4 | -4 | ([K2Cr2O7])^(-4) P_2S_5 | 1 | -1 | ([P2S5])^(-1) H_2O | 16 | 16 | ([H2O])^16 K_2SO_4 | 1 | 1 | [K2SO4] SO_2 | 8 | 8 | ([SO2])^8 Cr_2(SO_4)_3 | 4 | 4 | ([Cr2(SO4)3])^4 K3PO4 | 2 | 2 | ([K3PO4])^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])^(-16) ([K2Cr2O7])^(-4) ([P2S5])^(-1) ([H2O])^16 [K2SO4] ([SO2])^8 ([Cr2(SO4)3])^4 ([K3PO4])^2 = (([H2O])^16 [K2SO4] ([SO2])^8 ([Cr2(SO4)3])^4 ([K3PO4])^2)/(([H2SO4])^16 ([K2Cr2O7])^4 [P2S5])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + K_2Cr_2O_7 + P_2S_5 ⟶ H_2O + K_2SO_4 + SO_2 + Cr_2(SO_4)_3 + K3PO4 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: 16 H_2SO_4 + 4 K_2Cr_2O_7 + P_2S_5 ⟶ 16 H_2O + K_2SO_4 + 8 SO_2 + 4 Cr_2(SO_4)_3 + 2 K3PO4 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 | 16 | -16 K_2Cr_2O_7 | 4 | -4 P_2S_5 | 1 | -1 H_2O | 16 | 16 K_2SO_4 | 1 | 1 SO_2 | 8 | 8 Cr_2(SO_4)_3 | 4 | 4 K3PO4 | 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 | 16 | -16 | -1/16 (Δ[H2SO4])/(Δt) K_2Cr_2O_7 | 4 | -4 | -1/4 (Δ[K2Cr2O7])/(Δt) P_2S_5 | 1 | -1 | -(Δ[P2S5])/(Δt) H_2O | 16 | 16 | 1/16 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) SO_2 | 8 | 8 | 1/8 (Δ[SO2])/(Δt) Cr_2(SO_4)_3 | 4 | 4 | 1/4 (Δ[Cr2(SO4)3])/(Δt) K3PO4 | 2 | 2 | 1/2 (Δ[K3PO4])/(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 = -1/16 (Δ[H2SO4])/(Δt) = -1/4 (Δ[K2Cr2O7])/(Δt) = -(Δ[P2S5])/(Δt) = 1/16 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/8 (Δ[SO2])/(Δt) = 1/4 (Δ[Cr2(SO4)3])/(Δt) = 1/2 (Δ[K3PO4])/(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 + P_2S_5 ⟶ H_2O + K_2SO_4 + SO_2 + Cr_2(SO_4)_3 + K3PO4 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: 16 H_2SO_4 + 4 K_2Cr_2O_7 + P_2S_5 ⟶ 16 H_2O + K_2SO_4 + 8 SO_2 + 4 Cr_2(SO_4)_3 + 2 K3PO4 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 | 16 | -16 K_2Cr_2O_7 | 4 | -4 P_2S_5 | 1 | -1 H_2O | 16 | 16 K_2SO_4 | 1 | 1 SO_2 | 8 | 8 Cr_2(SO_4)_3 | 4 | 4 K3PO4 | 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 | 16 | -16 | -1/16 (Δ[H2SO4])/(Δt) K_2Cr_2O_7 | 4 | -4 | -1/4 (Δ[K2Cr2O7])/(Δt) P_2S_5 | 1 | -1 | -(Δ[P2S5])/(Δt) H_2O | 16 | 16 | 1/16 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) SO_2 | 8 | 8 | 1/8 (Δ[SO2])/(Δt) Cr_2(SO_4)_3 | 4 | 4 | 1/4 (Δ[Cr2(SO4)3])/(Δt) K3PO4 | 2 | 2 | 1/2 (Δ[K3PO4])/(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 = -1/16 (Δ[H2SO4])/(Δt) = -1/4 (Δ[K2Cr2O7])/(Δt) = -(Δ[P2S5])/(Δt) = 1/16 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/8 (Δ[SO2])/(Δt) = 1/4 (Δ[Cr2(SO4)3])/(Δt) = 1/2 (Δ[K3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium dichromate | phosphorus pentasulfide | water | potassium sulfate | sulfur dioxide | chromium sulfate | K3PO4 formula | H_2SO_4 | K_2Cr_2O_7 | P_2S_5 | H_2O | K_2SO_4 | SO_2 | Cr_2(SO_4)_3 | K3PO4 Hill formula | H_2O_4S | Cr_2K_2O_7 | P_2S_5 | H_2O | K_2O_4S | O_2S | Cr_2O_12S_3 | K3O4P name | sulfuric acid | potassium dichromate | phosphorus pentasulfide | water | potassium sulfate | sulfur dioxide | chromium sulfate | IUPAC name | sulfuric acid | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | | water | dipotassium sulfate | sulfur dioxide | chromium(+3) cation trisulfate |
| sulfuric acid | potassium dichromate | phosphorus pentasulfide | water | potassium sulfate | sulfur dioxide | chromium sulfate | K3PO4 formula | H_2SO_4 | K_2Cr_2O_7 | P_2S_5 | H_2O | K_2SO_4 | SO_2 | Cr_2(SO_4)_3 | K3PO4 Hill formula | H_2O_4S | Cr_2K_2O_7 | P_2S_5 | H_2O | K_2O_4S | O_2S | Cr_2O_12S_3 | K3O4P name | sulfuric acid | potassium dichromate | phosphorus pentasulfide | water | potassium sulfate | sulfur dioxide | chromium sulfate | IUPAC name | sulfuric acid | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | | water | dipotassium sulfate | sulfur dioxide | chromium(+3) cation trisulfate |

Random Queries

color of strontium CAS
discoverers of helium
chemical types of gallium(II) telluride
iron(III) oxide vs diphosphoryl chloride
tin(IV) cation vs cobalt(III) cation
PubChem CID number of carbon allotropes
empirical formula of barium titanate zirconate vs cobalt(II) formate dihydrate
molar mass of corundum
IUPAC name of sodium tungstate
find features image dioptase