Search

H2SO4 + KMnO4 + [Cr(NH2)2(CO)6]4[Cr(CN)6]3 = H2O + CO2 + K2SO4 + MnSO4 + K2Cr2O7 + KNO3

Input interpretation

H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O water + CO_2 carbon dioxide + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + K_2Cr_2O_7 potassium dichromate + KNO_3 potassium nitrate
H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O water + CO_2 carbon dioxide + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + K_2Cr_2O_7 potassium dichromate + KNO_3 potassium nitrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 + K_2Cr_2O_7 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ c_4 H_2O + c_5 CO_2 + c_6 K_2SO_4 + c_7 MnSO_4 + c_8 K_2Cr_2O_7 + c_9 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn, Cr, N and C: H: | 2 c_1 + 16 c_3 = 2 c_4 O: | 4 c_1 + 4 c_2 + 24 c_3 = c_4 + 2 c_5 + 4 c_6 + 4 c_7 + 7 c_8 + 3 c_9 S: | c_1 = c_6 + c_7 K: | c_2 = 2 c_6 + 2 c_8 + c_9 Mn: | c_2 = c_7 Cr: | 7 c_3 = 2 c_8 N: | 26 c_3 = c_9 C: | 42 c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 759/10 c_2 = 308/5 c_3 = 1 c_4 = 839/10 c_5 = 42 c_6 = 143/10 c_7 = 308/5 c_8 = 7/2 c_9 = 26 Multiply by the least common denominator, 10, to eliminate fractional coefficients: c_1 = 759 c_2 = 616 c_3 = 10 c_4 = 839 c_5 = 420 c_6 = 143 c_7 = 616 c_8 = 35 c_9 = 260 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 759 H_2SO_4 + 616 KMnO_4 + 10 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ 839 H_2O + 420 CO_2 + 143 K_2SO_4 + 616 MnSO_4 + 35 K_2Cr_2O_7 + 260 KNO_3
Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 + K_2Cr_2O_7 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ c_4 H_2O + c_5 CO_2 + c_6 K_2SO_4 + c_7 MnSO_4 + c_8 K_2Cr_2O_7 + c_9 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn, Cr, N and C: H: | 2 c_1 + 16 c_3 = 2 c_4 O: | 4 c_1 + 4 c_2 + 24 c_3 = c_4 + 2 c_5 + 4 c_6 + 4 c_7 + 7 c_8 + 3 c_9 S: | c_1 = c_6 + c_7 K: | c_2 = 2 c_6 + 2 c_8 + c_9 Mn: | c_2 = c_7 Cr: | 7 c_3 = 2 c_8 N: | 26 c_3 = c_9 C: | 42 c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 759/10 c_2 = 308/5 c_3 = 1 c_4 = 839/10 c_5 = 42 c_6 = 143/10 c_7 = 308/5 c_8 = 7/2 c_9 = 26 Multiply by the least common denominator, 10, to eliminate fractional coefficients: c_1 = 759 c_2 = 616 c_3 = 10 c_4 = 839 c_5 = 420 c_6 = 143 c_7 = 616 c_8 = 35 c_9 = 260 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 759 H_2SO_4 + 616 KMnO_4 + 10 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ 839 H_2O + 420 CO_2 + 143 K_2SO_4 + 616 MnSO_4 + 35 K_2Cr_2O_7 + 260 KNO_3

Structures

+ + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ + + + + +
+ + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ + + + + +

Names

sulfuric acid + potassium permanganate + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ water + carbon dioxide + potassium sulfate + manganese(II) sulfate + potassium dichromate + potassium nitrate
sulfuric acid + potassium permanganate + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ water + carbon dioxide + potassium sulfate + manganese(II) sulfate + potassium dichromate + potassium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 + K_2Cr_2O_7 + KNO_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: 759 H_2SO_4 + 616 KMnO_4 + 10 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ 839 H_2O + 420 CO_2 + 143 K_2SO_4 + 616 MnSO_4 + 35 K_2Cr_2O_7 + 260 KNO_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 | 759 | -759 KMnO_4 | 616 | -616 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 H_2O | 839 | 839 CO_2 | 420 | 420 K_2SO_4 | 143 | 143 MnSO_4 | 616 | 616 K_2Cr_2O_7 | 35 | 35 KNO_3 | 260 | 260 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 759 | -759 | ([H2SO4])^(-759) KMnO_4 | 616 | -616 | ([KMnO4])^(-616) (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 | ([(Cr(NH2)2(CO)6)4(Cr(CN)6)3])^(-10) H_2O | 839 | 839 | ([H2O])^839 CO_2 | 420 | 420 | ([CO2])^420 K_2SO_4 | 143 | 143 | ([K2SO4])^143 MnSO_4 | 616 | 616 | ([MnSO4])^616 K_2Cr_2O_7 | 35 | 35 | ([K2Cr2O7])^35 KNO_3 | 260 | 260 | ([KNO3])^260 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])^(-759) ([KMnO4])^(-616) ([(Cr(NH2)2(CO)6)4(Cr(CN)6)3])^(-10) ([H2O])^839 ([CO2])^420 ([K2SO4])^143 ([MnSO4])^616 ([K2Cr2O7])^35 ([KNO3])^260 = (([H2O])^839 ([CO2])^420 ([K2SO4])^143 ([MnSO4])^616 ([K2Cr2O7])^35 ([KNO3])^260)/(([H2SO4])^759 ([KMnO4])^616 ([(Cr(NH2)2(CO)6)4(Cr(CN)6)3])^10)
Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 + K_2Cr_2O_7 + KNO_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: 759 H_2SO_4 + 616 KMnO_4 + 10 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ 839 H_2O + 420 CO_2 + 143 K_2SO_4 + 616 MnSO_4 + 35 K_2Cr_2O_7 + 260 KNO_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 | 759 | -759 KMnO_4 | 616 | -616 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 H_2O | 839 | 839 CO_2 | 420 | 420 K_2SO_4 | 143 | 143 MnSO_4 | 616 | 616 K_2Cr_2O_7 | 35 | 35 KNO_3 | 260 | 260 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 759 | -759 | ([H2SO4])^(-759) KMnO_4 | 616 | -616 | ([KMnO4])^(-616) (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 | ([(Cr(NH2)2(CO)6)4(Cr(CN)6)3])^(-10) H_2O | 839 | 839 | ([H2O])^839 CO_2 | 420 | 420 | ([CO2])^420 K_2SO_4 | 143 | 143 | ([K2SO4])^143 MnSO_4 | 616 | 616 | ([MnSO4])^616 K_2Cr_2O_7 | 35 | 35 | ([K2Cr2O7])^35 KNO_3 | 260 | 260 | ([KNO3])^260 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])^(-759) ([KMnO4])^(-616) ([(Cr(NH2)2(CO)6)4(Cr(CN)6)3])^(-10) ([H2O])^839 ([CO2])^420 ([K2SO4])^143 ([MnSO4])^616 ([K2Cr2O7])^35 ([KNO3])^260 = (([H2O])^839 ([CO2])^420 ([K2SO4])^143 ([MnSO4])^616 ([K2Cr2O7])^35 ([KNO3])^260)/(([H2SO4])^759 ([KMnO4])^616 ([(Cr(NH2)2(CO)6)4(Cr(CN)6)3])^10)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 + K_2Cr_2O_7 + KNO_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: 759 H_2SO_4 + 616 KMnO_4 + 10 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ 839 H_2O + 420 CO_2 + 143 K_2SO_4 + 616 MnSO_4 + 35 K_2Cr_2O_7 + 260 KNO_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 | 759 | -759 KMnO_4 | 616 | -616 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 H_2O | 839 | 839 CO_2 | 420 | 420 K_2SO_4 | 143 | 143 MnSO_4 | 616 | 616 K_2Cr_2O_7 | 35 | 35 KNO_3 | 260 | 260 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 | 759 | -759 | -1/759 (Δ[H2SO4])/(Δt) KMnO_4 | 616 | -616 | -1/616 (Δ[KMnO4])/(Δt) (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 | -1/10 (Δ[(Cr(NH2)2(CO)6)4(Cr(CN)6)3])/(Δt) H_2O | 839 | 839 | 1/839 (Δ[H2O])/(Δt) CO_2 | 420 | 420 | 1/420 (Δ[CO2])/(Δt) K_2SO_4 | 143 | 143 | 1/143 (Δ[K2SO4])/(Δt) MnSO_4 | 616 | 616 | 1/616 (Δ[MnSO4])/(Δt) K_2Cr_2O_7 | 35 | 35 | 1/35 (Δ[K2Cr2O7])/(Δt) KNO_3 | 260 | 260 | 1/260 (Δ[KNO3])/(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 = -1/759 (Δ[H2SO4])/(Δt) = -1/616 (Δ[KMnO4])/(Δt) = -1/10 (Δ[(Cr(NH2)2(CO)6)4(Cr(CN)6)3])/(Δt) = 1/839 (Δ[H2O])/(Δt) = 1/420 (Δ[CO2])/(Δt) = 1/143 (Δ[K2SO4])/(Δt) = 1/616 (Δ[MnSO4])/(Δt) = 1/35 (Δ[K2Cr2O7])/(Δt) = 1/260 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 + K_2Cr_2O_7 + KNO_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: 759 H_2SO_4 + 616 KMnO_4 + 10 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 ⟶ 839 H_2O + 420 CO_2 + 143 K_2SO_4 + 616 MnSO_4 + 35 K_2Cr_2O_7 + 260 KNO_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 | 759 | -759 KMnO_4 | 616 | -616 (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 H_2O | 839 | 839 CO_2 | 420 | 420 K_2SO_4 | 143 | 143 MnSO_4 | 616 | 616 K_2Cr_2O_7 | 35 | 35 KNO_3 | 260 | 260 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 | 759 | -759 | -1/759 (Δ[H2SO4])/(Δt) KMnO_4 | 616 | -616 | -1/616 (Δ[KMnO4])/(Δt) (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | 10 | -10 | -1/10 (Δ[(Cr(NH2)2(CO)6)4(Cr(CN)6)3])/(Δt) H_2O | 839 | 839 | 1/839 (Δ[H2O])/(Δt) CO_2 | 420 | 420 | 1/420 (Δ[CO2])/(Δt) K_2SO_4 | 143 | 143 | 1/143 (Δ[K2SO4])/(Δt) MnSO_4 | 616 | 616 | 1/616 (Δ[MnSO4])/(Δt) K_2Cr_2O_7 | 35 | 35 | 1/35 (Δ[K2Cr2O7])/(Δt) KNO_3 | 260 | 260 | 1/260 (Δ[KNO3])/(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 = -1/759 (Δ[H2SO4])/(Δt) = -1/616 (Δ[KMnO4])/(Δt) = -1/10 (Δ[(Cr(NH2)2(CO)6)4(Cr(CN)6)3])/(Δt) = 1/839 (Δ[H2O])/(Δt) = 1/420 (Δ[CO2])/(Δt) = 1/143 (Δ[K2SO4])/(Δt) = 1/616 (Δ[MnSO4])/(Δt) = 1/35 (Δ[K2Cr2O7])/(Δt) = 1/260 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium permanganate | (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | water | carbon dioxide | potassium sulfate | manganese(II) sulfate | potassium dichromate | potassium nitrate formula | H_2SO_4 | KMnO_4 | (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | H_2O | CO_2 | K_2SO_4 | MnSO_4 | K_2Cr_2O_7 | KNO_3 Hill formula | H_2O_4S | KMnO_4 | C42H16Cr7N26O24 | H_2O | CO_2 | K_2O_4S | MnSO_4 | Cr_2K_2O_7 | KNO_3 name | sulfuric acid | potassium permanganate | | water | carbon dioxide | potassium sulfate | manganese(II) sulfate | potassium dichromate | potassium nitrate IUPAC name | sulfuric acid | potassium permanganate | | water | carbon dioxide | dipotassium sulfate | manganese(+2) cation sulfate | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | potassium nitrate
| sulfuric acid | potassium permanganate | (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | water | carbon dioxide | potassium sulfate | manganese(II) sulfate | potassium dichromate | potassium nitrate formula | H_2SO_4 | KMnO_4 | (Cr(NH2)2(CO)6)4(Cr(CN)6)3 | H_2O | CO_2 | K_2SO_4 | MnSO_4 | K_2Cr_2O_7 | KNO_3 Hill formula | H_2O_4S | KMnO_4 | C42H16Cr7N26O24 | H_2O | CO_2 | K_2O_4S | MnSO_4 | Cr_2K_2O_7 | KNO_3 name | sulfuric acid | potassium permanganate | | water | carbon dioxide | potassium sulfate | manganese(II) sulfate | potassium dichromate | potassium nitrate IUPAC name | sulfuric acid | potassium permanganate | | water | carbon dioxide | dipotassium sulfate | manganese(+2) cation sulfate | dipotassium oxido-(oxido-dioxochromio)oxy-dioxochromium | potassium nitrate

Random Queries

van der Waals radius hydrogen
H2SO4 + BeO = H2O + BeSO4
IUPAC name of 1,4-bis(trifluoromethyl)benzene-13 C6 vs 1,1,2,2-tetrafluoroethane
H-bond acceptor count of stannous chloride vs stannous oxide
formula of halogenated
melting point of fluoxetine
calcium selenate dihydrate
chemical types sodium hypochlorite
crystal class of diamond vs chromium
Curie point of group 10 elements