Search

Cu(NO3)2 + P2O3 = NO + CuO + P2O5

Input interpretation

Cu(NO_3)_2 copper(II) nitrate + P_2O_3 phosphorus trioxide ⟶ NO nitric oxide + CuO cupric oxide + P2O5
Cu(NO_3)_2 copper(II) nitrate + P_2O_3 phosphorus trioxide ⟶ NO nitric oxide + CuO cupric oxide + P2O5

Balanced equation

Balance the chemical equation algebraically: Cu(NO_3)_2 + P_2O_3 ⟶ NO + CuO + P2O5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu(NO_3)_2 + c_2 P_2O_3 ⟶ c_3 NO + c_4 CuO + c_5 P2O5 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, N, O and P: Cu: | c_1 = c_4 N: | 2 c_1 = c_3 O: | 6 c_1 + 3 c_2 = c_3 + c_4 + 5 c_5 P: | 2 c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3/2 c_3 = 2 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 4 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Cu(NO_3)_2 + 3 P_2O_3 ⟶ 4 NO + 2 CuO + 3 P2O5
Balance the chemical equation algebraically: Cu(NO_3)_2 + P_2O_3 ⟶ NO + CuO + P2O5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu(NO_3)_2 + c_2 P_2O_3 ⟶ c_3 NO + c_4 CuO + c_5 P2O5 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, N, O and P: Cu: | c_1 = c_4 N: | 2 c_1 = c_3 O: | 6 c_1 + 3 c_2 = c_3 + c_4 + 5 c_5 P: | 2 c_2 = 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3/2 c_3 = 2 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 2 c_2 = 3 c_3 = 4 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 Cu(NO_3)_2 + 3 P_2O_3 ⟶ 4 NO + 2 CuO + 3 P2O5

Structures

+ ⟶ + + P2O5
+ ⟶ + + P2O5

Names

copper(II) nitrate + phosphorus trioxide ⟶ nitric oxide + cupric oxide + P2O5
copper(II) nitrate + phosphorus trioxide ⟶ nitric oxide + cupric oxide + P2O5

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cu(NO_3)_2 + P_2O_3 ⟶ NO + CuO + P2O5 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 Cu(NO_3)_2 + 3 P_2O_3 ⟶ 4 NO + 2 CuO + 3 P2O5 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 Cu(NO_3)_2 | 2 | -2 P_2O_3 | 3 | -3 NO | 4 | 4 CuO | 2 | 2 P2O5 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cu(NO_3)_2 | 2 | -2 | ([Cu(NO3)2])^(-2) P_2O_3 | 3 | -3 | ([P2O3])^(-3) NO | 4 | 4 | ([NO])^4 CuO | 2 | 2 | ([CuO])^2 P2O5 | 3 | 3 | ([P2O5])^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 = ([Cu(NO3)2])^(-2) ([P2O3])^(-3) ([NO])^4 ([CuO])^2 ([P2O5])^3 = (([NO])^4 ([CuO])^2 ([P2O5])^3)/(([Cu(NO3)2])^2 ([P2O3])^3)
Construct the equilibrium constant, K, expression for: Cu(NO_3)_2 + P_2O_3 ⟶ NO + CuO + P2O5 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 Cu(NO_3)_2 + 3 P_2O_3 ⟶ 4 NO + 2 CuO + 3 P2O5 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 Cu(NO_3)_2 | 2 | -2 P_2O_3 | 3 | -3 NO | 4 | 4 CuO | 2 | 2 P2O5 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cu(NO_3)_2 | 2 | -2 | ([Cu(NO3)2])^(-2) P_2O_3 | 3 | -3 | ([P2O3])^(-3) NO | 4 | 4 | ([NO])^4 CuO | 2 | 2 | ([CuO])^2 P2O5 | 3 | 3 | ([P2O5])^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 = ([Cu(NO3)2])^(-2) ([P2O3])^(-3) ([NO])^4 ([CuO])^2 ([P2O5])^3 = (([NO])^4 ([CuO])^2 ([P2O5])^3)/(([Cu(NO3)2])^2 ([P2O3])^3)

Rate of reaction

Construct the rate of reaction expression for: Cu(NO_3)_2 + P_2O_3 ⟶ NO + CuO + P2O5 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 Cu(NO_3)_2 + 3 P_2O_3 ⟶ 4 NO + 2 CuO + 3 P2O5 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 Cu(NO_3)_2 | 2 | -2 P_2O_3 | 3 | -3 NO | 4 | 4 CuO | 2 | 2 P2O5 | 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 Cu(NO_3)_2 | 2 | -2 | -1/2 (Δ[Cu(NO3)2])/(Δt) P_2O_3 | 3 | -3 | -1/3 (Δ[P2O3])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(Δt) CuO | 2 | 2 | 1/2 (Δ[CuO])/(Δt) P2O5 | 3 | 3 | 1/3 (Δ[P2O5])/(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[Cu(NO3)2])/(Δt) = -1/3 (Δ[P2O3])/(Δt) = 1/4 (Δ[NO])/(Δt) = 1/2 (Δ[CuO])/(Δt) = 1/3 (Δ[P2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cu(NO_3)_2 + P_2O_3 ⟶ NO + CuO + P2O5 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 Cu(NO_3)_2 + 3 P_2O_3 ⟶ 4 NO + 2 CuO + 3 P2O5 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 Cu(NO_3)_2 | 2 | -2 P_2O_3 | 3 | -3 NO | 4 | 4 CuO | 2 | 2 P2O5 | 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 Cu(NO_3)_2 | 2 | -2 | -1/2 (Δ[Cu(NO3)2])/(Δt) P_2O_3 | 3 | -3 | -1/3 (Δ[P2O3])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(Δt) CuO | 2 | 2 | 1/2 (Δ[CuO])/(Δt) P2O5 | 3 | 3 | 1/3 (Δ[P2O5])/(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[Cu(NO3)2])/(Δt) = -1/3 (Δ[P2O3])/(Δt) = 1/4 (Δ[NO])/(Δt) = 1/2 (Δ[CuO])/(Δt) = 1/3 (Δ[P2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| copper(II) nitrate | phosphorus trioxide | nitric oxide | cupric oxide | P2O5 formula | Cu(NO_3)_2 | P_2O_3 | NO | CuO | P2O5 Hill formula | CuN_2O_6 | O_3P_2 | NO | CuO | O5P2 name | copper(II) nitrate | phosphorus trioxide | nitric oxide | cupric oxide |
| copper(II) nitrate | phosphorus trioxide | nitric oxide | cupric oxide | P2O5 formula | Cu(NO_3)_2 | P_2O_3 | NO | CuO | P2O5 Hill formula | CuN_2O_6 | O_3P_2 | NO | CuO | O5P2 name | copper(II) nitrate | phosphorus trioxide | nitric oxide | cupric oxide |

Substance properties

| copper(II) nitrate | phosphorus trioxide | nitric oxide | cupric oxide | P2O5 molar mass | 187.55 g/mol | 109.94 g/mol | 30.006 g/mol | 79.545 g/mol | 141.94 g/mol phase | | solid (at STP) | gas (at STP) | solid (at STP) | melting point | | 23.8 °C | -163.6 °C | 1326 °C | boiling point | | 173.1 °C | -151.7 °C | 2000 °C | density | | 2.135 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 6.315 g/cm^3 | solubility in water | | decomposes | | insoluble | dynamic viscosity | | | 1.911×10^-5 Pa s (at 25 °C) | |
| copper(II) nitrate | phosphorus trioxide | nitric oxide | cupric oxide | P2O5 molar mass | 187.55 g/mol | 109.94 g/mol | 30.006 g/mol | 79.545 g/mol | 141.94 g/mol phase | | solid (at STP) | gas (at STP) | solid (at STP) | melting point | | 23.8 °C | -163.6 °C | 1326 °C | boiling point | | 173.1 °C | -151.7 °C | 2000 °C | density | | 2.135 g/cm^3 | 0.001226 g/cm^3 (at 25 °C) | 6.315 g/cm^3 | solubility in water | | decomposes | | insoluble | dynamic viscosity | | | 1.911×10^-5 Pa s (at 25 °C) | |

Units

Random Queries

atomic radius of barium vs ytterbium
chemical types nitrogen
CAS number of iodine monochloride vs magnesium oxide
apply charcoal effect to image ofmellite
non-standard isotope numbers of ethylamine
formula of sodium formate vs gallium(III) oxide
ion class of osmium(VI) cation vs fluoride anion
marr edges image sylvite
boiling point of potassium fluoride
barium iodate monohydrate