Search

Ca(OH)2 + P4O10 = H2O + CaHPO4

Input interpretation

Ca(OH)_2 calcium hydroxide + P_4O_10 phosphorus pentoxide ⟶ H_2O water + CaHPO_4 calcium hydrogen phosphate
Ca(OH)_2 calcium hydroxide + P_4O_10 phosphorus pentoxide ⟶ H_2O water + CaHPO_4 calcium hydrogen phosphate

Balanced equation

Balance the chemical equation algebraically: Ca(OH)_2 + P_4O_10 ⟶ H_2O + CaHPO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 P_4O_10 ⟶ c_3 H_2O + c_4 CaHPO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O and P: Ca: | c_1 = c_4 H: | 2 c_1 = 2 c_3 + c_4 O: | 2 c_1 + 10 c_2 = c_3 + 4 c_4 P: | 4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 2 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 Ca(OH)_2 + P_4O_10 ⟶ 2 H_2O + 4 CaHPO_4
Balance the chemical equation algebraically: Ca(OH)_2 + P_4O_10 ⟶ H_2O + CaHPO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 P_4O_10 ⟶ c_3 H_2O + c_4 CaHPO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O and P: Ca: | c_1 = c_4 H: | 2 c_1 = 2 c_3 + c_4 O: | 2 c_1 + 10 c_2 = c_3 + 4 c_4 P: | 4 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 2 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 Ca(OH)_2 + P_4O_10 ⟶ 2 H_2O + 4 CaHPO_4

Structures

+ ⟶ +
+ ⟶ +

Names

calcium hydroxide + phosphorus pentoxide ⟶ water + calcium hydrogen phosphate
calcium hydroxide + phosphorus pentoxide ⟶ water + calcium hydrogen phosphate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Ca(OH)_2 + P_4O_10 ⟶ H_2O + CaHPO_4 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: 4 Ca(OH)_2 + P_4O_10 ⟶ 2 H_2O + 4 CaHPO_4 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 Ca(OH)_2 | 4 | -4 P_4O_10 | 1 | -1 H_2O | 2 | 2 CaHPO_4 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(OH)_2 | 4 | -4 | ([Ca(OH)2])^(-4) P_4O_10 | 1 | -1 | ([P4O10])^(-1) H_2O | 2 | 2 | ([H2O])^2 CaHPO_4 | 4 | 4 | ([CaHPO4])^4 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 = ([Ca(OH)2])^(-4) ([P4O10])^(-1) ([H2O])^2 ([CaHPO4])^4 = (([H2O])^2 ([CaHPO4])^4)/(([Ca(OH)2])^4 [P4O10])
Construct the equilibrium constant, K, expression for: Ca(OH)_2 + P_4O_10 ⟶ H_2O + CaHPO_4 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: 4 Ca(OH)_2 + P_4O_10 ⟶ 2 H_2O + 4 CaHPO_4 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 Ca(OH)_2 | 4 | -4 P_4O_10 | 1 | -1 H_2O | 2 | 2 CaHPO_4 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(OH)_2 | 4 | -4 | ([Ca(OH)2])^(-4) P_4O_10 | 1 | -1 | ([P4O10])^(-1) H_2O | 2 | 2 | ([H2O])^2 CaHPO_4 | 4 | 4 | ([CaHPO4])^4 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 = ([Ca(OH)2])^(-4) ([P4O10])^(-1) ([H2O])^2 ([CaHPO4])^4 = (([H2O])^2 ([CaHPO4])^4)/(([Ca(OH)2])^4 [P4O10])

Rate of reaction

Construct the rate of reaction expression for: Ca(OH)_2 + P_4O_10 ⟶ H_2O + CaHPO_4 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: 4 Ca(OH)_2 + P_4O_10 ⟶ 2 H_2O + 4 CaHPO_4 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 Ca(OH)_2 | 4 | -4 P_4O_10 | 1 | -1 H_2O | 2 | 2 CaHPO_4 | 4 | 4 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 Ca(OH)_2 | 4 | -4 | -1/4 (Δ[Ca(OH)2])/(Δt) P_4O_10 | 1 | -1 | -(Δ[P4O10])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) CaHPO_4 | 4 | 4 | 1/4 (Δ[CaHPO4])/(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 = -1/4 (Δ[Ca(OH)2])/(Δt) = -(Δ[P4O10])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/4 (Δ[CaHPO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Ca(OH)_2 + P_4O_10 ⟶ H_2O + CaHPO_4 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: 4 Ca(OH)_2 + P_4O_10 ⟶ 2 H_2O + 4 CaHPO_4 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 Ca(OH)_2 | 4 | -4 P_4O_10 | 1 | -1 H_2O | 2 | 2 CaHPO_4 | 4 | 4 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 Ca(OH)_2 | 4 | -4 | -1/4 (Δ[Ca(OH)2])/(Δt) P_4O_10 | 1 | -1 | -(Δ[P4O10])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) CaHPO_4 | 4 | 4 | 1/4 (Δ[CaHPO4])/(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 = -1/4 (Δ[Ca(OH)2])/(Δt) = -(Δ[P4O10])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/4 (Δ[CaHPO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| calcium hydroxide | phosphorus pentoxide | water | calcium hydrogen phosphate formula | Ca(OH)_2 | P_4O_10 | H_2O | CaHPO_4 Hill formula | CaH_2O_2 | O_10P_4 | H_2O | CaHO_4P name | calcium hydroxide | phosphorus pentoxide | water | calcium hydrogen phosphate IUPAC name | calcium dihydroxide | | water | calcium hydroxy-dioxido-oxo-phosphorane
| calcium hydroxide | phosphorus pentoxide | water | calcium hydrogen phosphate formula | Ca(OH)_2 | P_4O_10 | H_2O | CaHPO_4 Hill formula | CaH_2O_2 | O_10P_4 | H_2O | CaHO_4P name | calcium hydroxide | phosphorus pentoxide | water | calcium hydrogen phosphate IUPAC name | calcium dihydroxide | | water | calcium hydroxy-dioxido-oxo-phosphorane

Substance properties

| calcium hydroxide | phosphorus pentoxide | water | calcium hydrogen phosphate molar mass | 74.092 g/mol | 283.89 g/mol | 18.015 g/mol | 136.06 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 550 °C | 340 °C | 0 °C | 370 °C boiling point | | | 99.9839 °C | density | 2.24 g/cm^3 | 2.3 g/cm^3 | 1 g/cm^3 | 2.89 g/cm^3 solubility in water | slightly soluble | | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |
| calcium hydroxide | phosphorus pentoxide | water | calcium hydrogen phosphate molar mass | 74.092 g/mol | 283.89 g/mol | 18.015 g/mol | 136.06 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 550 °C | 340 °C | 0 °C | 370 °C boiling point | | | 99.9839 °C | density | 2.24 g/cm^3 | 2.3 g/cm^3 | 1 g/cm^3 | 2.89 g/cm^3 solubility in water | slightly soluble | | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |

Units

Random Queries

color of actinium vs plutonium
NaOH + BeO = H2O + Na2BeO2
maximum common substructure of atp and caffeine
chemical types of platinum(IV) oxide vs tetrabutylphosphonium bromide
PubChem CID number of 1-methylbutylzinc bromide
Hildebrand solubility parameter of polar protic solvents
chemical types of lithium zirconate vs 4-fluorobenzylzinc chloride
ions of silver(I) carbonate vs magnesium molybdate
count of ammonium
luster of acuminite vs chloroxiphite