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CuO + HN3 = H2O + Cu + N2

Input interpretation

CuO cupric oxide + HNN congruent N hydrazoic acid ⟶ H_2O water + Cu copper + N_2 nitrogen
CuO cupric oxide + HNN congruent N hydrazoic acid ⟶ H_2O water + Cu copper + N_2 nitrogen

Balanced equation

Balance the chemical equation algebraically: CuO + HNN congruent N ⟶ H_2O + Cu + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 HNN congruent N ⟶ c_3 H_2O + c_4 Cu + c_5 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, H and N: Cu: | c_1 = c_4 O: | c_1 = c_3 H: | c_2 = 2 c_3 N: | 3 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 = 2 c_3 = 1 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuO + 2 HNN congruent N ⟶ H_2O + Cu + 3 N_2
Balance the chemical equation algebraically: CuO + HNN congruent N ⟶ H_2O + Cu + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuO + c_2 HNN congruent N ⟶ c_3 H_2O + c_4 Cu + c_5 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, H and N: Cu: | c_1 = c_4 O: | c_1 = c_3 H: | c_2 = 2 c_3 N: | 3 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 = 2 c_3 = 1 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CuO + 2 HNN congruent N ⟶ H_2O + Cu + 3 N_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

cupric oxide + hydrazoic acid ⟶ water + copper + nitrogen
cupric oxide + hydrazoic acid ⟶ water + copper + nitrogen

Equilibrium constant

Construct the equilibrium constant, K, expression for: CuO + HNN congruent N ⟶ H_2O + Cu + N_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: CuO + 2 HNN congruent N ⟶ H_2O + Cu + 3 N_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 CuO | 1 | -1 HNN congruent N | 2 | -2 H_2O | 1 | 1 Cu | 1 | 1 N_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 1 | -1 | ([CuO])^(-1) HNN congruent N | 2 | -2 | ([HNN congruent N])^(-2) H_2O | 1 | 1 | [H2O] Cu | 1 | 1 | [Cu] N_2 | 3 | 3 | ([N2])^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 = ([CuO])^(-1) ([HNN congruent N])^(-2) [H2O] [Cu] ([N2])^3 = ([H2O] [Cu] ([N2])^3)/([CuO] ([HNN congruent N])^2)
Construct the equilibrium constant, K, expression for: CuO + HNN congruent N ⟶ H_2O + Cu + N_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: CuO + 2 HNN congruent N ⟶ H_2O + Cu + 3 N_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 CuO | 1 | -1 HNN congruent N | 2 | -2 H_2O | 1 | 1 Cu | 1 | 1 N_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuO | 1 | -1 | ([CuO])^(-1) HNN congruent N | 2 | -2 | ([HNN congruent N])^(-2) H_2O | 1 | 1 | [H2O] Cu | 1 | 1 | [Cu] N_2 | 3 | 3 | ([N2])^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 = ([CuO])^(-1) ([HNN congruent N])^(-2) [H2O] [Cu] ([N2])^3 = ([H2O] [Cu] ([N2])^3)/([CuO] ([HNN congruent N])^2)

Rate of reaction

Construct the rate of reaction expression for: CuO + HNN congruent N ⟶ H_2O + Cu + N_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: CuO + 2 HNN congruent N ⟶ H_2O + Cu + 3 N_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 CuO | 1 | -1 HNN congruent N | 2 | -2 H_2O | 1 | 1 Cu | 1 | 1 N_2 | 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 CuO | 1 | -1 | -(Δ[CuO])/(Δt) HNN congruent N | 2 | -2 | -1/2 (Δ[HNN congruent N])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(Δt) N_2 | 3 | 3 | 1/3 (Δ[N2])/(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 = -(Δ[CuO])/(Δt) = -1/2 (Δ[HNN congruent N])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cu])/(Δt) = 1/3 (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CuO + HNN congruent N ⟶ H_2O + Cu + N_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: CuO + 2 HNN congruent N ⟶ H_2O + Cu + 3 N_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 CuO | 1 | -1 HNN congruent N | 2 | -2 H_2O | 1 | 1 Cu | 1 | 1 N_2 | 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 CuO | 1 | -1 | -(Δ[CuO])/(Δt) HNN congruent N | 2 | -2 | -1/2 (Δ[HNN congruent N])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) Cu | 1 | 1 | (Δ[Cu])/(Δt) N_2 | 3 | 3 | 1/3 (Δ[N2])/(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 = -(Δ[CuO])/(Δt) = -1/2 (Δ[HNN congruent N])/(Δt) = (Δ[H2O])/(Δt) = (Δ[Cu])/(Δt) = 1/3 (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| cupric oxide | hydrazoic acid | water | copper | nitrogen formula | CuO | HNN congruent N | H_2O | Cu | N_2 Hill formula | CuO | HN_3 | H_2O | Cu | N_2 name | cupric oxide | hydrazoic acid | water | copper | nitrogen IUPAC name | | diazonioazanide | water | copper | molecular nitrogen
| cupric oxide | hydrazoic acid | water | copper | nitrogen formula | CuO | HNN congruent N | H_2O | Cu | N_2 Hill formula | CuO | HN_3 | H_2O | Cu | N_2 name | cupric oxide | hydrazoic acid | water | copper | nitrogen IUPAC name | | diazonioazanide | water | copper | molecular nitrogen

Substance properties

| cupric oxide | hydrazoic acid | water | copper | nitrogen molar mass | 79.545 g/mol | 43.029 g/mol | 18.015 g/mol | 63.546 g/mol | 28.014 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) melting point | 1326 °C | | 0 °C | 1083 °C | -210 °C boiling point | 2000 °C | | 99.9839 °C | 2567 °C | -195.79 °C density | 6.315 g/cm^3 | | 1 g/cm^3 | 8.96 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | insoluble | | | insoluble | insoluble surface tension | | | 0.0728 N/m | | 0.0066 N/m dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | odorless | odorless | odorless
| cupric oxide | hydrazoic acid | water | copper | nitrogen molar mass | 79.545 g/mol | 43.029 g/mol | 18.015 g/mol | 63.546 g/mol | 28.014 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) melting point | 1326 °C | | 0 °C | 1083 °C | -210 °C boiling point | 2000 °C | | 99.9839 °C | 2567 °C | -195.79 °C density | 6.315 g/cm^3 | | 1 g/cm^3 | 8.96 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | insoluble | | | insoluble | insoluble surface tension | | | 0.0728 N/m | | 0.0066 N/m dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | odorless | odorless | odorless

Units

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