Search

H2O + O2 + Au + KCN = KOH + KAu(CN)3

Input interpretation

H_2O water + O_2 oxygen + Au gold + KCN potassium cyanide ⟶ KOH potassium hydroxide + KAu(CN)3
H_2O water + O_2 oxygen + Au gold + KCN potassium cyanide ⟶ KOH potassium hydroxide + KAu(CN)3

Balanced equation

Balance the chemical equation algebraically: H_2O + O_2 + Au + KCN ⟶ KOH + KAu(CN)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 O_2 + c_3 Au + c_4 KCN ⟶ c_5 KOH + c_6 KAu(CN)3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Au, C, K and N: H: | 2 c_1 = c_5 O: | c_1 + 2 c_2 = c_5 Au: | c_3 = c_6 C: | c_4 = 3 c_6 K: | c_4 = c_5 + c_6 N: | c_4 = 3 c_6 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 = 2 c_4 = 6 c_5 = 4 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + O_2 + 2 Au + 6 KCN ⟶ 4 KOH + 2 KAu(CN)3
Balance the chemical equation algebraically: H_2O + O_2 + Au + KCN ⟶ KOH + KAu(CN)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 O_2 + c_3 Au + c_4 KCN ⟶ c_5 KOH + c_6 KAu(CN)3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Au, C, K and N: H: | 2 c_1 = c_5 O: | c_1 + 2 c_2 = c_5 Au: | c_3 = c_6 C: | c_4 = 3 c_6 K: | c_4 = c_5 + c_6 N: | c_4 = 3 c_6 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 = 2 c_4 = 6 c_5 = 4 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + O_2 + 2 Au + 6 KCN ⟶ 4 KOH + 2 KAu(CN)3

Structures

+ + + ⟶ + KAu(CN)3
+ + + ⟶ + KAu(CN)3

Names

water + oxygen + gold + potassium cyanide ⟶ potassium hydroxide + KAu(CN)3
water + oxygen + gold + potassium cyanide ⟶ potassium hydroxide + KAu(CN)3

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + O_2 + Au + KCN ⟶ KOH + KAu(CN)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: 2 H_2O + O_2 + 2 Au + 6 KCN ⟶ 4 KOH + 2 KAu(CN)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_2O | 2 | -2 O_2 | 1 | -1 Au | 2 | -2 KCN | 6 | -6 KOH | 4 | 4 KAu(CN)3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) O_2 | 1 | -1 | ([O2])^(-1) Au | 2 | -2 | ([Au])^(-2) KCN | 6 | -6 | ([KCN])^(-6) KOH | 4 | 4 | ([KOH])^4 KAu(CN)3 | 2 | 2 | ([KAu(CN)3])^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 = ([H2O])^(-2) ([O2])^(-1) ([Au])^(-2) ([KCN])^(-6) ([KOH])^4 ([KAu(CN)3])^2 = (([KOH])^4 ([KAu(CN)3])^2)/(([H2O])^2 [O2] ([Au])^2 ([KCN])^6)
Construct the equilibrium constant, K, expression for: H_2O + O_2 + Au + KCN ⟶ KOH + KAu(CN)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: 2 H_2O + O_2 + 2 Au + 6 KCN ⟶ 4 KOH + 2 KAu(CN)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_2O | 2 | -2 O_2 | 1 | -1 Au | 2 | -2 KCN | 6 | -6 KOH | 4 | 4 KAu(CN)3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) O_2 | 1 | -1 | ([O2])^(-1) Au | 2 | -2 | ([Au])^(-2) KCN | 6 | -6 | ([KCN])^(-6) KOH | 4 | 4 | ([KOH])^4 KAu(CN)3 | 2 | 2 | ([KAu(CN)3])^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 = ([H2O])^(-2) ([O2])^(-1) ([Au])^(-2) ([KCN])^(-6) ([KOH])^4 ([KAu(CN)3])^2 = (([KOH])^4 ([KAu(CN)3])^2)/(([H2O])^2 [O2] ([Au])^2 ([KCN])^6)

Rate of reaction

Construct the rate of reaction expression for: H_2O + O_2 + Au + KCN ⟶ KOH + KAu(CN)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: 2 H_2O + O_2 + 2 Au + 6 KCN ⟶ 4 KOH + 2 KAu(CN)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_2O | 2 | -2 O_2 | 1 | -1 Au | 2 | -2 KCN | 6 | -6 KOH | 4 | 4 KAu(CN)3 | 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) O_2 | 1 | -1 | -(Δ[O2])/(Δt) Au | 2 | -2 | -1/2 (Δ[Au])/(Δt) KCN | 6 | -6 | -1/6 (Δ[KCN])/(Δt) KOH | 4 | 4 | 1/4 (Δ[KOH])/(Δt) KAu(CN)3 | 2 | 2 | 1/2 (Δ[KAu(CN)3])/(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[H2O])/(Δt) = -(Δ[O2])/(Δt) = -1/2 (Δ[Au])/(Δt) = -1/6 (Δ[KCN])/(Δt) = 1/4 (Δ[KOH])/(Δt) = 1/2 (Δ[KAu(CN)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + O_2 + Au + KCN ⟶ KOH + KAu(CN)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: 2 H_2O + O_2 + 2 Au + 6 KCN ⟶ 4 KOH + 2 KAu(CN)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_2O | 2 | -2 O_2 | 1 | -1 Au | 2 | -2 KCN | 6 | -6 KOH | 4 | 4 KAu(CN)3 | 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) O_2 | 1 | -1 | -(Δ[O2])/(Δt) Au | 2 | -2 | -1/2 (Δ[Au])/(Δt) KCN | 6 | -6 | -1/6 (Δ[KCN])/(Δt) KOH | 4 | 4 | 1/4 (Δ[KOH])/(Δt) KAu(CN)3 | 2 | 2 | 1/2 (Δ[KAu(CN)3])/(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[H2O])/(Δt) = -(Δ[O2])/(Δt) = -1/2 (Δ[Au])/(Δt) = -1/6 (Δ[KCN])/(Δt) = 1/4 (Δ[KOH])/(Δt) = 1/2 (Δ[KAu(CN)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | oxygen | gold | potassium cyanide | potassium hydroxide | KAu(CN)3 formula | H_2O | O_2 | Au | KCN | KOH | KAu(CN)3 Hill formula | H_2O | O_2 | Au | CKN | HKO | C3AuKN3 name | water | oxygen | gold | potassium cyanide | potassium hydroxide | IUPAC name | water | molecular oxygen | gold | potassium cyanide | potassium hydroxide |
| water | oxygen | gold | potassium cyanide | potassium hydroxide | KAu(CN)3 formula | H_2O | O_2 | Au | KCN | KOH | KAu(CN)3 Hill formula | H_2O | O_2 | Au | CKN | HKO | C3AuKN3 name | water | oxygen | gold | potassium cyanide | potassium hydroxide | IUPAC name | water | molecular oxygen | gold | potassium cyanide | potassium hydroxide |

Substance properties

| water | oxygen | gold | potassium cyanide | potassium hydroxide | KAu(CN)3 molar mass | 18.015 g/mol | 31.998 g/mol | 196.966569 g/mol | 65.116 g/mol | 56.105 g/mol | 314.119 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | | solid (at STP) | melting point | 0 °C | -218 °C | 1063 °C | | 406 °C | boiling point | 99.9839 °C | -183 °C | 2856 °C | | 1327 °C | density | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 19.3 g/cm^3 | | 2.044 g/cm^3 | solubility in water | | | insoluble | | soluble | surface tension | 0.0728 N/m | 0.01347 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | | | 0.001 Pa s (at 550 °C) | odor | odorless | odorless | | | |
| water | oxygen | gold | potassium cyanide | potassium hydroxide | KAu(CN)3 molar mass | 18.015 g/mol | 31.998 g/mol | 196.966569 g/mol | 65.116 g/mol | 56.105 g/mol | 314.119 g/mol phase | liquid (at STP) | gas (at STP) | solid (at STP) | | solid (at STP) | melting point | 0 °C | -218 °C | 1063 °C | | 406 °C | boiling point | 99.9839 °C | -183 °C | 2856 °C | | 1327 °C | density | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 19.3 g/cm^3 | | 2.044 g/cm^3 | solubility in water | | | insoluble | | soluble | surface tension | 0.0728 N/m | 0.01347 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | | | 0.001 Pa s (at 550 °C) | odor | odorless | odorless | | | |

Units

Random Queries

density of iodine bromide
formula string of zinc cation vs nitrate anion
freezing point of deuterium hydride
net ionic charge of vanadium(IV) cation
atomic number of fluorine
formula of aluminum chloride vs magnesium sulfite hexahydrate
H2 + Rb = RbH
Mohs hardness of bytownite
PubChem CID number of sertraline
chemical uses methyl chloride