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H2O + NH3 + Cu(NO3)2 = NH4NO3 + Cu(OH)2

Input interpretation

H_2O water + NH_3 ammonia + Cu(NO_3)_2 copper(II) nitrate ⟶ NH_4NO_3 ammonium nitrate + Cu(OH)_2 copper hydroxide
H_2O water + NH_3 ammonia + Cu(NO_3)_2 copper(II) nitrate ⟶ NH_4NO_3 ammonium nitrate + Cu(OH)_2 copper hydroxide

Balanced equation

Balance the chemical equation algebraically: H_2O + NH_3 + Cu(NO_3)_2 ⟶ NH_4NO_3 + Cu(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NH_3 + c_3 Cu(NO_3)_2 ⟶ c_4 NH_4NO_3 + c_5 Cu(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and Cu: H: | 2 c_1 + 3 c_2 = 4 c_4 + 2 c_5 O: | c_1 + 6 c_3 = 3 c_4 + 2 c_5 N: | c_2 + 2 c_3 = 2 c_4 Cu: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 NH_3 + Cu(NO_3)_2 ⟶ 2 NH_4NO_3 + Cu(OH)_2
Balance the chemical equation algebraically: H_2O + NH_3 + Cu(NO_3)_2 ⟶ NH_4NO_3 + Cu(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 NH_3 + c_3 Cu(NO_3)_2 ⟶ c_4 NH_4NO_3 + c_5 Cu(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N and Cu: H: | 2 c_1 + 3 c_2 = 4 c_4 + 2 c_5 O: | c_1 + 6 c_3 = 3 c_4 + 2 c_5 N: | c_2 + 2 c_3 = 2 c_4 Cu: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 NH_3 + Cu(NO_3)_2 ⟶ 2 NH_4NO_3 + Cu(OH)_2

Structures

+ + ⟶ +
+ + ⟶ +

Names

water + ammonia + copper(II) nitrate ⟶ ammonium nitrate + copper hydroxide
water + ammonia + copper(II) nitrate ⟶ ammonium nitrate + copper hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + NH_3 + Cu(NO_3)_2 ⟶ NH_4NO_3 + Cu(OH)_2 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 + 2 NH_3 + Cu(NO_3)_2 ⟶ 2 NH_4NO_3 + Cu(OH)_2 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 NH_3 | 2 | -2 Cu(NO_3)_2 | 1 | -1 NH_4NO_3 | 2 | 2 Cu(OH)_2 | 1 | 1 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) NH_3 | 2 | -2 | ([NH3])^(-2) Cu(NO_3)_2 | 1 | -1 | ([Cu(NO3)2])^(-1) NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 Cu(OH)_2 | 1 | 1 | [Cu(OH)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) ([NH3])^(-2) ([Cu(NO3)2])^(-1) ([NH4NO3])^2 [Cu(OH)2] = (([NH4NO3])^2 [Cu(OH)2])/(([H2O])^2 ([NH3])^2 [Cu(NO3)2])
Construct the equilibrium constant, K, expression for: H_2O + NH_3 + Cu(NO_3)_2 ⟶ NH_4NO_3 + Cu(OH)_2 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 + 2 NH_3 + Cu(NO_3)_2 ⟶ 2 NH_4NO_3 + Cu(OH)_2 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 NH_3 | 2 | -2 Cu(NO_3)_2 | 1 | -1 NH_4NO_3 | 2 | 2 Cu(OH)_2 | 1 | 1 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) NH_3 | 2 | -2 | ([NH3])^(-2) Cu(NO_3)_2 | 1 | -1 | ([Cu(NO3)2])^(-1) NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 Cu(OH)_2 | 1 | 1 | [Cu(OH)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) ([NH3])^(-2) ([Cu(NO3)2])^(-1) ([NH4NO3])^2 [Cu(OH)2] = (([NH4NO3])^2 [Cu(OH)2])/(([H2O])^2 ([NH3])^2 [Cu(NO3)2])

Rate of reaction

Construct the rate of reaction expression for: H_2O + NH_3 + Cu(NO_3)_2 ⟶ NH_4NO_3 + Cu(OH)_2 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 + 2 NH_3 + Cu(NO_3)_2 ⟶ 2 NH_4NO_3 + Cu(OH)_2 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 NH_3 | 2 | -2 Cu(NO_3)_2 | 1 | -1 NH_4NO_3 | 2 | 2 Cu(OH)_2 | 1 | 1 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) NH_3 | 2 | -2 | -1/2 (Δ[NH3])/(Δt) Cu(NO_3)_2 | 1 | -1 | -(Δ[Cu(NO3)2])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(Δt) Cu(OH)_2 | 1 | 1 | (Δ[Cu(OH)2])/(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) = -1/2 (Δ[NH3])/(Δt) = -(Δ[Cu(NO3)2])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) = (Δ[Cu(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + NH_3 + Cu(NO_3)_2 ⟶ NH_4NO_3 + Cu(OH)_2 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 + 2 NH_3 + Cu(NO_3)_2 ⟶ 2 NH_4NO_3 + Cu(OH)_2 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 NH_3 | 2 | -2 Cu(NO_3)_2 | 1 | -1 NH_4NO_3 | 2 | 2 Cu(OH)_2 | 1 | 1 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) NH_3 | 2 | -2 | -1/2 (Δ[NH3])/(Δt) Cu(NO_3)_2 | 1 | -1 | -(Δ[Cu(NO3)2])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(Δt) Cu(OH)_2 | 1 | 1 | (Δ[Cu(OH)2])/(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) = -1/2 (Δ[NH3])/(Δt) = -(Δ[Cu(NO3)2])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) = (Δ[Cu(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | ammonia | copper(II) nitrate | ammonium nitrate | copper hydroxide formula | H_2O | NH_3 | Cu(NO_3)_2 | NH_4NO_3 | Cu(OH)_2 Hill formula | H_2O | H_3N | CuN_2O_6 | H_4N_2O_3 | CuH_2O_2 name | water | ammonia | copper(II) nitrate | ammonium nitrate | copper hydroxide IUPAC name | water | ammonia | copper(II) nitrate | | copper dihydroxide
| water | ammonia | copper(II) nitrate | ammonium nitrate | copper hydroxide formula | H_2O | NH_3 | Cu(NO_3)_2 | NH_4NO_3 | Cu(OH)_2 Hill formula | H_2O | H_3N | CuN_2O_6 | H_4N_2O_3 | CuH_2O_2 name | water | ammonia | copper(II) nitrate | ammonium nitrate | copper hydroxide IUPAC name | water | ammonia | copper(II) nitrate | | copper dihydroxide

Substance properties

| water | ammonia | copper(II) nitrate | ammonium nitrate | copper hydroxide molar mass | 18.015 g/mol | 17.031 g/mol | 187.55 g/mol | 80.04 g/mol | 97.56 g/mol phase | liquid (at STP) | gas (at STP) | | solid (at STP) | melting point | 0 °C | -77.73 °C | | 169 °C | boiling point | 99.9839 °C | -33.33 °C | | 210 °C | density | 1 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | | 1.73 g/cm^3 | surface tension | 0.0728 N/m | 0.0234 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.009×10^-5 Pa s (at 25 °C) | | | odor | odorless | | | odorless |
| water | ammonia | copper(II) nitrate | ammonium nitrate | copper hydroxide molar mass | 18.015 g/mol | 17.031 g/mol | 187.55 g/mol | 80.04 g/mol | 97.56 g/mol phase | liquid (at STP) | gas (at STP) | | solid (at STP) | melting point | 0 °C | -77.73 °C | | 169 °C | boiling point | 99.9839 °C | -33.33 °C | | 210 °C | density | 1 g/cm^3 | 6.96×10^-4 g/cm^3 (at 25 °C) | | 1.73 g/cm^3 | surface tension | 0.0728 N/m | 0.0234 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.009×10^-5 Pa s (at 25 °C) | | | odor | odorless | | | odorless |

Units

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