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H2SO4 + AlP = Al2(SO4)3 + PH3

Input interpretation

H_2SO_4 sulfuric acid + AlP aluminum phosphide ⟶ Al_2(SO_4)_3 aluminum sulfate + PH_3 phosphine
H_2SO_4 sulfuric acid + AlP aluminum phosphide ⟶ Al_2(SO_4)_3 aluminum sulfate + PH_3 phosphine

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + AlP ⟶ Al_2(SO_4)_3 + PH_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 AlP ⟶ c_3 Al_2(SO_4)_3 + c_4 PH_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Al and P: H: | 2 c_1 = 3 c_4 O: | 4 c_1 = 12 c_3 S: | c_1 = 3 c_3 Al: | c_2 = 2 c_3 P: | c_2 = c_4 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 = 3 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 2 AlP ⟶ Al_2(SO_4)_3 + 2 PH_3
Balance the chemical equation algebraically: H_2SO_4 + AlP ⟶ Al_2(SO_4)_3 + PH_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 AlP ⟶ c_3 Al_2(SO_4)_3 + c_4 PH_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Al and P: H: | 2 c_1 = 3 c_4 O: | 4 c_1 = 12 c_3 S: | c_1 = 3 c_3 Al: | c_2 = 2 c_3 P: | c_2 = c_4 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 = 3 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 2 AlP ⟶ Al_2(SO_4)_3 + 2 PH_3

Structures

+ ⟶ +
+ ⟶ +

Names

sulfuric acid + aluminum phosphide ⟶ aluminum sulfate + phosphine
sulfuric acid + aluminum phosphide ⟶ aluminum sulfate + phosphine

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + AlP ⟶ Al_2(SO_4)_3 + PH_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: 3 H_2SO_4 + 2 AlP ⟶ Al_2(SO_4)_3 + 2 PH_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 | 3 | -3 AlP | 2 | -2 Al_2(SO_4)_3 | 1 | 1 PH_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_2SO_4 | 3 | -3 | ([H2SO4])^(-3) AlP | 2 | -2 | ([AlP])^(-2) Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] PH_3 | 2 | 2 | ([PH3])^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])^(-3) ([AlP])^(-2) [Al2(SO4)3] ([PH3])^2 = ([Al2(SO4)3] ([PH3])^2)/(([H2SO4])^3 ([AlP])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + AlP ⟶ Al_2(SO_4)_3 + PH_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: 3 H_2SO_4 + 2 AlP ⟶ Al_2(SO_4)_3 + 2 PH_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 | 3 | -3 AlP | 2 | -2 Al_2(SO_4)_3 | 1 | 1 PH_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_2SO_4 | 3 | -3 | ([H2SO4])^(-3) AlP | 2 | -2 | ([AlP])^(-2) Al_2(SO_4)_3 | 1 | 1 | [Al2(SO4)3] PH_3 | 2 | 2 | ([PH3])^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])^(-3) ([AlP])^(-2) [Al2(SO4)3] ([PH3])^2 = ([Al2(SO4)3] ([PH3])^2)/(([H2SO4])^3 ([AlP])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + AlP ⟶ Al_2(SO_4)_3 + PH_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: 3 H_2SO_4 + 2 AlP ⟶ Al_2(SO_4)_3 + 2 PH_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 | 3 | -3 AlP | 2 | -2 Al_2(SO_4)_3 | 1 | 1 PH_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_2SO_4 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) AlP | 2 | -2 | -1/2 (Δ[AlP])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(Δt) PH_3 | 2 | 2 | 1/2 (Δ[PH3])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -1/2 (Δ[AlP])/(Δt) = (Δ[Al2(SO4)3])/(Δt) = 1/2 (Δ[PH3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + AlP ⟶ Al_2(SO_4)_3 + PH_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: 3 H_2SO_4 + 2 AlP ⟶ Al_2(SO_4)_3 + 2 PH_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 | 3 | -3 AlP | 2 | -2 Al_2(SO_4)_3 | 1 | 1 PH_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_2SO_4 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) AlP | 2 | -2 | -1/2 (Δ[AlP])/(Δt) Al_2(SO_4)_3 | 1 | 1 | (Δ[Al2(SO4)3])/(Δt) PH_3 | 2 | 2 | 1/2 (Δ[PH3])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -1/2 (Δ[AlP])/(Δt) = (Δ[Al2(SO4)3])/(Δt) = 1/2 (Δ[PH3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | aluminum phosphide | aluminum sulfate | phosphine formula | H_2SO_4 | AlP | Al_2(SO_4)_3 | PH_3 Hill formula | H_2O_4S | AlP | Al_2O_12S_3 | H_3P name | sulfuric acid | aluminum phosphide | aluminum sulfate | phosphine IUPAC name | sulfuric acid | alumanylidynephosphane | dialuminum trisulfate | phosphine
| sulfuric acid | aluminum phosphide | aluminum sulfate | phosphine formula | H_2SO_4 | AlP | Al_2(SO_4)_3 | PH_3 Hill formula | H_2O_4S | AlP | Al_2O_12S_3 | H_3P name | sulfuric acid | aluminum phosphide | aluminum sulfate | phosphine IUPAC name | sulfuric acid | alumanylidynephosphane | dialuminum trisulfate | phosphine

Substance properties

| sulfuric acid | aluminum phosphide | aluminum sulfate | phosphine molar mass | 98.07 g/mol | 57.9553005 g/mol | 342.1 g/mol | 33.998 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) melting point | 10.371 °C | 2530 °C | 770 °C | -132.8 °C boiling point | 279.6 °C | | | -87.5 °C density | 1.8305 g/cm^3 | 2.85 g/cm^3 | 2.71 g/cm^3 | 0.00139 g/cm^3 (at 25 °C) solubility in water | very soluble | reacts | soluble | slightly soluble surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | 1.1×10^-5 Pa s (at 0 °C) odor | odorless | | |
| sulfuric acid | aluminum phosphide | aluminum sulfate | phosphine molar mass | 98.07 g/mol | 57.9553005 g/mol | 342.1 g/mol | 33.998 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) melting point | 10.371 °C | 2530 °C | 770 °C | -132.8 °C boiling point | 279.6 °C | | | -87.5 °C density | 1.8305 g/cm^3 | 2.85 g/cm^3 | 2.71 g/cm^3 | 0.00139 g/cm^3 (at 25 °C) solubility in water | very soluble | reacts | soluble | slightly soluble surface tension | 0.0735 N/m | | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | | 1.1×10^-5 Pa s (at 0 °C) odor | odorless | | |

Units

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