Input interpretation
![O_2 (oxygen) + Hg (mercury) ⟶ HgO (mercuric oxide)](../image_source/69b5c38da83362e5e15bdc7c8b6be77d.png)
O_2 (oxygen) + Hg (mercury) ⟶ HgO (mercuric oxide)
Balanced equation
![Balance the chemical equation algebraically: O_2 + Hg ⟶ HgO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Hg ⟶ c_3 HgO Set the number of atoms in the reactants equal to the number of atoms in the products for O and Hg: O: | 2 c_1 = c_3 Hg: | c_2 = c_3 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | O_2 + 2 Hg ⟶ 2 HgO](../image_source/d354e8fc084a5400d7c4441bb8753a4c.png)
Balance the chemical equation algebraically: O_2 + Hg ⟶ HgO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Hg ⟶ c_3 HgO Set the number of atoms in the reactants equal to the number of atoms in the products for O and Hg: O: | 2 c_1 = c_3 Hg: | c_2 = c_3 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 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | O_2 + 2 Hg ⟶ 2 HgO
Structures
![+ ⟶](../image_source/dbe7bb794c97f116ad66ea719c14c3a8.png)
+ ⟶
Names
![oxygen + mercury ⟶ mercuric oxide](../image_source/07e6f9be6c33d84220f1227202bd230c.png)
oxygen + mercury ⟶ mercuric oxide
Reaction thermodynamics
Enthalpy
![| oxygen | mercury | mercuric oxide molecular enthalpy | 0 kJ/mol | 0 kJ/mol | -90 kJ/mol total enthalpy | 0 kJ/mol | 0 kJ/mol | -180 kJ/mol | H_initial = 0 kJ/mol | | H_final = -180 kJ/mol ΔH_rxn^0 | -180 kJ/mol - 0 kJ/mol = -180 kJ/mol (exothermic) | |](../image_source/8b21d26b3ee32e6e5de73fd7bed0c28e.png)
| oxygen | mercury | mercuric oxide molecular enthalpy | 0 kJ/mol | 0 kJ/mol | -90 kJ/mol total enthalpy | 0 kJ/mol | 0 kJ/mol | -180 kJ/mol | H_initial = 0 kJ/mol | | H_final = -180 kJ/mol ΔH_rxn^0 | -180 kJ/mol - 0 kJ/mol = -180 kJ/mol (exothermic) | |
Gibbs free energy
![| oxygen | mercury | mercuric oxide molecular free energy | 231.7 kJ/mol | 0 kJ/mol | -59 kJ/mol total free energy | 231.7 kJ/mol | 0 kJ/mol | -118 kJ/mol | G_initial = 231.7 kJ/mol | | G_final = -118 kJ/mol ΔG_rxn^0 | -118 kJ/mol - 231.7 kJ/mol = -349.7 kJ/mol (exergonic) | |](../image_source/293782b1b42edfe0538f62f9397e20c2.png)
| oxygen | mercury | mercuric oxide molecular free energy | 231.7 kJ/mol | 0 kJ/mol | -59 kJ/mol total free energy | 231.7 kJ/mol | 0 kJ/mol | -118 kJ/mol | G_initial = 231.7 kJ/mol | | G_final = -118 kJ/mol ΔG_rxn^0 | -118 kJ/mol - 231.7 kJ/mol = -349.7 kJ/mol (exergonic) | |
Entropy
![| oxygen | mercury | mercuric oxide molecular entropy | 205 J/(mol K) | 76 J/(mol K) | 70 J/(mol K) total entropy | 205 J/(mol K) | 152 J/(mol K) | 140 J/(mol K) | S_initial = 357 J/(mol K) | | S_final = 140 J/(mol K) ΔS_rxn^0 | 140 J/(mol K) - 357 J/(mol K) = -217 J/(mol K) (exoentropic) | |](../image_source/4315c935473ed287824fd32643742fab.png)
| oxygen | mercury | mercuric oxide molecular entropy | 205 J/(mol K) | 76 J/(mol K) | 70 J/(mol K) total entropy | 205 J/(mol K) | 152 J/(mol K) | 140 J/(mol K) | S_initial = 357 J/(mol K) | | S_final = 140 J/(mol K) ΔS_rxn^0 | 140 J/(mol K) - 357 J/(mol K) = -217 J/(mol K) (exoentropic) | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: O_2 + Hg ⟶ HgO 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: O_2 + 2 Hg ⟶ 2 HgO 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 O_2 | 1 | -1 Hg | 2 | -2 HgO | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 1 | -1 | ([O2])^(-1) Hg | 2 | -2 | ([Hg])^(-2) HgO | 2 | 2 | ([HgO])^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 = ([O2])^(-1) ([Hg])^(-2) ([HgO])^2 = ([HgO])^2/([O2] ([Hg])^2)](../image_source/a043b7f6716f1565cd6f018f1332ae68.png)
Construct the equilibrium constant, K, expression for: O_2 + Hg ⟶ HgO 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: O_2 + 2 Hg ⟶ 2 HgO 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 O_2 | 1 | -1 Hg | 2 | -2 HgO | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression O_2 | 1 | -1 | ([O2])^(-1) Hg | 2 | -2 | ([Hg])^(-2) HgO | 2 | 2 | ([HgO])^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 = ([O2])^(-1) ([Hg])^(-2) ([HgO])^2 = ([HgO])^2/([O2] ([Hg])^2)
Rate of reaction
![Construct the rate of reaction expression for: O_2 + Hg ⟶ HgO 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: O_2 + 2 Hg ⟶ 2 HgO 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 O_2 | 1 | -1 Hg | 2 | -2 HgO | 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 O_2 | 1 | -1 | -(Δ[O2])/(Δt) Hg | 2 | -2 | -1/2 (Δ[Hg])/(Δt) HgO | 2 | 2 | 1/2 (Δ[HgO])/(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[O2])/(Δt) = -1/2 (Δ[Hg])/(Δt) = 1/2 (Δ[HgO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/bed9c331e62768fce1eb94b721b7603e.png)
Construct the rate of reaction expression for: O_2 + Hg ⟶ HgO 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: O_2 + 2 Hg ⟶ 2 HgO 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 O_2 | 1 | -1 Hg | 2 | -2 HgO | 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 O_2 | 1 | -1 | -(Δ[O2])/(Δt) Hg | 2 | -2 | -1/2 (Δ[Hg])/(Δt) HgO | 2 | 2 | 1/2 (Δ[HgO])/(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[O2])/(Δt) = -1/2 (Δ[Hg])/(Δt) = 1/2 (Δ[HgO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| oxygen | mercury | mercuric oxide formula | O_2 | Hg | HgO name | oxygen | mercury | mercuric oxide IUPAC name | molecular oxygen | mercury | oxomercury](../image_source/eee29121651e0dc107419eae83598b9b.png)
| oxygen | mercury | mercuric oxide formula | O_2 | Hg | HgO name | oxygen | mercury | mercuric oxide IUPAC name | molecular oxygen | mercury | oxomercury
Substance properties
![| oxygen | mercury | mercuric oxide molar mass | 31.998 g/mol | 200.592 g/mol | 216.591 g/mol phase | gas (at STP) | liquid (at STP) | solid (at STP) melting point | -218 °C | -38.87 °C | 500 °C boiling point | -183 °C | 356.6 °C | density | 0.001429 g/cm^3 (at 0 °C) | 13.534 g/cm^3 | 11.14 g/cm^3 solubility in water | | slightly soluble | insoluble surface tension | 0.01347 N/m | 0.47 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 0.001526 Pa s (at 25 °C) | odor | odorless | odorless | odorless](../image_source/295d8ae625f9c4362ab04706275a1f55.png)
| oxygen | mercury | mercuric oxide molar mass | 31.998 g/mol | 200.592 g/mol | 216.591 g/mol phase | gas (at STP) | liquid (at STP) | solid (at STP) melting point | -218 °C | -38.87 °C | 500 °C boiling point | -183 °C | 356.6 °C | density | 0.001429 g/cm^3 (at 0 °C) | 13.534 g/cm^3 | 11.14 g/cm^3 solubility in water | | slightly soluble | insoluble surface tension | 0.01347 N/m | 0.47 N/m | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | 0.001526 Pa s (at 25 °C) | odor | odorless | odorless | odorless
Units