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H2O + Cu(NO3)2 = O2 + HNO3 + Cu

Input interpretation

H_2O water + Cu(NO_3)_2 copper(II) nitrate ⟶ O_2 oxygen + HNO_3 nitric acid + Cu copper
H_2O water + Cu(NO_3)_2 copper(II) nitrate ⟶ O_2 oxygen + HNO_3 nitric acid + Cu copper

Balanced equation

Balance the chemical equation algebraically: H_2O + Cu(NO_3)_2 ⟶ O_2 + HNO_3 + Cu Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cu(NO_3)_2 ⟶ c_3 O_2 + c_4 HNO_3 + c_5 Cu Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cu and N: H: | 2 c_1 = c_4 O: | c_1 + 6 c_2 = 2 c_3 + 3 c_4 Cu: | c_2 = c_5 N: | 2 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 = 2 c_2 = 2 c_3 = 1 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 Cu(NO_3)_2 ⟶ O_2 + 4 HNO_3 + 2 Cu
Balance the chemical equation algebraically: H_2O + Cu(NO_3)_2 ⟶ O_2 + HNO_3 + Cu Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cu(NO_3)_2 ⟶ c_3 O_2 + c_4 HNO_3 + c_5 Cu Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Cu and N: H: | 2 c_1 = c_4 O: | c_1 + 6 c_2 = 2 c_3 + 3 c_4 Cu: | c_2 = c_5 N: | 2 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 = 2 c_2 = 2 c_3 = 1 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 Cu(NO_3)_2 ⟶ O_2 + 4 HNO_3 + 2 Cu

Structures

+ ⟶ + +
+ ⟶ + +

Names

water + copper(II) nitrate ⟶ oxygen + nitric acid + copper
water + copper(II) nitrate ⟶ oxygen + nitric acid + copper

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Cu(NO_3)_2 ⟶ O_2 + HNO_3 + Cu 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 Cu(NO_3)_2 ⟶ O_2 + 4 HNO_3 + 2 Cu 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 Cu(NO_3)_2 | 2 | -2 O_2 | 1 | 1 HNO_3 | 4 | 4 Cu | 2 | 2 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) Cu(NO_3)_2 | 2 | -2 | ([Cu(NO3)2])^(-2) O_2 | 1 | 1 | [O2] HNO_3 | 4 | 4 | ([HNO3])^4 Cu | 2 | 2 | ([Cu])^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) ([Cu(NO3)2])^(-2) [O2] ([HNO3])^4 ([Cu])^2 = ([O2] ([HNO3])^4 ([Cu])^2)/(([H2O])^2 ([Cu(NO3)2])^2)
Construct the equilibrium constant, K, expression for: H_2O + Cu(NO_3)_2 ⟶ O_2 + HNO_3 + Cu 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 Cu(NO_3)_2 ⟶ O_2 + 4 HNO_3 + 2 Cu 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 Cu(NO_3)_2 | 2 | -2 O_2 | 1 | 1 HNO_3 | 4 | 4 Cu | 2 | 2 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) Cu(NO_3)_2 | 2 | -2 | ([Cu(NO3)2])^(-2) O_2 | 1 | 1 | [O2] HNO_3 | 4 | 4 | ([HNO3])^4 Cu | 2 | 2 | ([Cu])^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) ([Cu(NO3)2])^(-2) [O2] ([HNO3])^4 ([Cu])^2 = ([O2] ([HNO3])^4 ([Cu])^2)/(([H2O])^2 ([Cu(NO3)2])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2O + Cu(NO_3)_2 ⟶ O_2 + HNO_3 + Cu 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 Cu(NO_3)_2 ⟶ O_2 + 4 HNO_3 + 2 Cu 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 Cu(NO_3)_2 | 2 | -2 O_2 | 1 | 1 HNO_3 | 4 | 4 Cu | 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) Cu(NO_3)_2 | 2 | -2 | -1/2 (Δ[Cu(NO3)2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) HNO_3 | 4 | 4 | 1/4 (Δ[HNO3])/(Δt) Cu | 2 | 2 | 1/2 (Δ[Cu])/(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[Cu(NO3)2])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[HNO3])/(Δt) = 1/2 (Δ[Cu])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Cu(NO_3)_2 ⟶ O_2 + HNO_3 + Cu 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 Cu(NO_3)_2 ⟶ O_2 + 4 HNO_3 + 2 Cu 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 Cu(NO_3)_2 | 2 | -2 O_2 | 1 | 1 HNO_3 | 4 | 4 Cu | 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) Cu(NO_3)_2 | 2 | -2 | -1/2 (Δ[Cu(NO3)2])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) HNO_3 | 4 | 4 | 1/4 (Δ[HNO3])/(Δt) Cu | 2 | 2 | 1/2 (Δ[Cu])/(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[Cu(NO3)2])/(Δt) = (Δ[O2])/(Δt) = 1/4 (Δ[HNO3])/(Δt) = 1/2 (Δ[Cu])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | copper(II) nitrate | oxygen | nitric acid | copper formula | H_2O | Cu(NO_3)_2 | O_2 | HNO_3 | Cu Hill formula | H_2O | CuN_2O_6 | O_2 | HNO_3 | Cu name | water | copper(II) nitrate | oxygen | nitric acid | copper IUPAC name | water | copper(II) nitrate | molecular oxygen | nitric acid | copper
| water | copper(II) nitrate | oxygen | nitric acid | copper formula | H_2O | Cu(NO_3)_2 | O_2 | HNO_3 | Cu Hill formula | H_2O | CuN_2O_6 | O_2 | HNO_3 | Cu name | water | copper(II) nitrate | oxygen | nitric acid | copper IUPAC name | water | copper(II) nitrate | molecular oxygen | nitric acid | copper

Substance properties

| water | copper(II) nitrate | oxygen | nitric acid | copper molar mass | 18.015 g/mol | 187.55 g/mol | 31.998 g/mol | 63.012 g/mol | 63.546 g/mol phase | liquid (at STP) | | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 0 °C | | -218 °C | -41.6 °C | 1083 °C boiling point | 99.9839 °C | | -183 °C | 83 °C | 2567 °C density | 1 g/cm^3 | | 0.001429 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 8.96 g/cm^3 solubility in water | | | | miscible | insoluble surface tension | 0.0728 N/m | | 0.01347 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 2.055×10^-5 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless | | odorless
| water | copper(II) nitrate | oxygen | nitric acid | copper molar mass | 18.015 g/mol | 187.55 g/mol | 31.998 g/mol | 63.012 g/mol | 63.546 g/mol phase | liquid (at STP) | | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 0 °C | | -218 °C | -41.6 °C | 1083 °C boiling point | 99.9839 °C | | -183 °C | 83 °C | 2567 °C density | 1 g/cm^3 | | 0.001429 g/cm^3 (at 0 °C) | 1.5129 g/cm^3 | 8.96 g/cm^3 solubility in water | | | | miscible | insoluble surface tension | 0.0728 N/m | | 0.01347 N/m | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 2.055×10^-5 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless | | odorless

Units

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