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H2O + KOH + P = PH3 + KH2PO3

Input interpretation

H_2O water + KOH potassium hydroxide + P red phosphorus ⟶ PH_3 phosphine + KH_2PO_3 potassium dihydrogen phospho nate
H_2O water + KOH potassium hydroxide + P red phosphorus ⟶ PH_3 phosphine + KH_2PO_3 potassium dihydrogen phospho nate

Balanced equation

Balance the chemical equation algebraically: H_2O + KOH + P ⟶ PH_3 + KH_2PO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KOH + c_3 P ⟶ c_4 PH_3 + c_5 KH_2PO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K and P: H: | 2 c_1 + c_2 = 3 c_4 + 3 c_5 O: | c_1 + c_2 = 3 c_5 K: | c_2 = c_5 P: | c_3 = c_4 + 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 3/2 c_3 = 5/2 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 3 c_3 = 5 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 H_2O + 3 KOH + 5 P ⟶ 2 PH_3 + 3 KH_2PO_3
Balance the chemical equation algebraically: H_2O + KOH + P ⟶ PH_3 + KH_2PO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KOH + c_3 P ⟶ c_4 PH_3 + c_5 KH_2PO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K and P: H: | 2 c_1 + c_2 = 3 c_4 + 3 c_5 O: | c_1 + c_2 = 3 c_5 K: | c_2 = c_5 P: | c_3 = c_4 + 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 3/2 c_3 = 5/2 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 6 c_2 = 3 c_3 = 5 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 H_2O + 3 KOH + 5 P ⟶ 2 PH_3 + 3 KH_2PO_3

Structures

+ + ⟶ +
+ + ⟶ +

Names

water + potassium hydroxide + red phosphorus ⟶ phosphine + potassium dihydrogen phospho nate
water + potassium hydroxide + red phosphorus ⟶ phosphine + potassium dihydrogen phospho nate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + KOH + P ⟶ PH_3 + KH_2PO_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: 6 H_2O + 3 KOH + 5 P ⟶ 2 PH_3 + 3 KH_2PO_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 | 6 | -6 KOH | 3 | -3 P | 5 | -5 PH_3 | 2 | 2 KH_2PO_3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 6 | -6 | ([H2O])^(-6) KOH | 3 | -3 | ([KOH])^(-3) P | 5 | -5 | ([P])^(-5) PH_3 | 2 | 2 | ([PH3])^2 KH_2PO_3 | 3 | 3 | ([KH2PO3])^3 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])^(-6) ([KOH])^(-3) ([P])^(-5) ([PH3])^2 ([KH2PO3])^3 = (([PH3])^2 ([KH2PO3])^3)/(([H2O])^6 ([KOH])^3 ([P])^5)
Construct the equilibrium constant, K, expression for: H_2O + KOH + P ⟶ PH_3 + KH_2PO_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: 6 H_2O + 3 KOH + 5 P ⟶ 2 PH_3 + 3 KH_2PO_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 | 6 | -6 KOH | 3 | -3 P | 5 | -5 PH_3 | 2 | 2 KH_2PO_3 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 6 | -6 | ([H2O])^(-6) KOH | 3 | -3 | ([KOH])^(-3) P | 5 | -5 | ([P])^(-5) PH_3 | 2 | 2 | ([PH3])^2 KH_2PO_3 | 3 | 3 | ([KH2PO3])^3 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])^(-6) ([KOH])^(-3) ([P])^(-5) ([PH3])^2 ([KH2PO3])^3 = (([PH3])^2 ([KH2PO3])^3)/(([H2O])^6 ([KOH])^3 ([P])^5)

Rate of reaction

Construct the rate of reaction expression for: H_2O + KOH + P ⟶ PH_3 + KH_2PO_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: 6 H_2O + 3 KOH + 5 P ⟶ 2 PH_3 + 3 KH_2PO_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 | 6 | -6 KOH | 3 | -3 P | 5 | -5 PH_3 | 2 | 2 KH_2PO_3 | 3 | 3 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 | 6 | -6 | -1/6 (Δ[H2O])/(Δt) KOH | 3 | -3 | -1/3 (Δ[KOH])/(Δt) P | 5 | -5 | -1/5 (Δ[P])/(Δt) PH_3 | 2 | 2 | 1/2 (Δ[PH3])/(Δt) KH_2PO_3 | 3 | 3 | 1/3 (Δ[KH2PO3])/(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 = -1/6 (Δ[H2O])/(Δt) = -1/3 (Δ[KOH])/(Δt) = -1/5 (Δ[P])/(Δt) = 1/2 (Δ[PH3])/(Δt) = 1/3 (Δ[KH2PO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + KOH + P ⟶ PH_3 + KH_2PO_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: 6 H_2O + 3 KOH + 5 P ⟶ 2 PH_3 + 3 KH_2PO_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 | 6 | -6 KOH | 3 | -3 P | 5 | -5 PH_3 | 2 | 2 KH_2PO_3 | 3 | 3 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 | 6 | -6 | -1/6 (Δ[H2O])/(Δt) KOH | 3 | -3 | -1/3 (Δ[KOH])/(Δt) P | 5 | -5 | -1/5 (Δ[P])/(Δt) PH_3 | 2 | 2 | 1/2 (Δ[PH3])/(Δt) KH_2PO_3 | 3 | 3 | 1/3 (Δ[KH2PO3])/(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 = -1/6 (Δ[H2O])/(Δt) = -1/3 (Δ[KOH])/(Δt) = -1/5 (Δ[P])/(Δt) = 1/2 (Δ[PH3])/(Δt) = 1/3 (Δ[KH2PO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | potassium hydroxide | red phosphorus | phosphine | potassium dihydrogen phospho nate formula | H_2O | KOH | P | PH_3 | KH_2PO_3 Hill formula | H_2O | HKO | P | H_3P | H_2KO_3P name | water | potassium hydroxide | red phosphorus | phosphine | potassium dihydrogen phospho nate IUPAC name | water | potassium hydroxide | phosphorus | phosphine |
| water | potassium hydroxide | red phosphorus | phosphine | potassium dihydrogen phospho nate formula | H_2O | KOH | P | PH_3 | KH_2PO_3 Hill formula | H_2O | HKO | P | H_3P | H_2KO_3P name | water | potassium hydroxide | red phosphorus | phosphine | potassium dihydrogen phospho nate IUPAC name | water | potassium hydroxide | phosphorus | phosphine |

Substance properties

| water | potassium hydroxide | red phosphorus | phosphine | potassium dihydrogen phospho nate molar mass | 18.015 g/mol | 56.105 g/mol | 30.973761998 g/mol | 33.998 g/mol | 121.09 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) | melting point | 0 °C | 406 °C | 579.2 °C | -132.8 °C | boiling point | 99.9839 °C | 1327 °C | | -87.5 °C | density | 1 g/cm^3 | 2.044 g/cm^3 | 2.16 g/cm^3 | 0.00139 g/cm^3 (at 25 °C) | solubility in water | | soluble | insoluble | slightly soluble | surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | 7.6×10^-4 Pa s (at 20.2 °C) | 1.1×10^-5 Pa s (at 0 °C) | odor | odorless | | | |
| water | potassium hydroxide | red phosphorus | phosphine | potassium dihydrogen phospho nate molar mass | 18.015 g/mol | 56.105 g/mol | 30.973761998 g/mol | 33.998 g/mol | 121.09 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) | melting point | 0 °C | 406 °C | 579.2 °C | -132.8 °C | boiling point | 99.9839 °C | 1327 °C | | -87.5 °C | density | 1 g/cm^3 | 2.044 g/cm^3 | 2.16 g/cm^3 | 0.00139 g/cm^3 (at 25 °C) | solubility in water | | soluble | insoluble | slightly soluble | surface tension | 0.0728 N/m | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | 7.6×10^-4 Pa s (at 20.2 °C) | 1.1×10^-5 Pa s (at 0 °C) | odor | odorless | | | |

Units

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