Input interpretation
![O_2 oxygen + Mn manganese ⟶ MnO manganese monoxide](../image_source/0d2ac7d374b76a890638783911fa114c.png)
O_2 oxygen + Mn manganese ⟶ MnO manganese monoxide
Balanced equation
![Balance the chemical equation algebraically: O_2 + Mn ⟶ MnO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Mn ⟶ c_3 MnO Set the number of atoms in the reactants equal to the number of atoms in the products for O and Mn: O: | 2 c_1 = c_3 Mn: | 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 Mn ⟶ 2 MnO](../image_source/95cb45aacb302265f00c50fad95bbb52.png)
Balance the chemical equation algebraically: O_2 + Mn ⟶ MnO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 O_2 + c_2 Mn ⟶ c_3 MnO Set the number of atoms in the reactants equal to the number of atoms in the products for O and Mn: O: | 2 c_1 = c_3 Mn: | 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 Mn ⟶ 2 MnO
Structures
![+ ⟶](../image_source/bf7ce593e584debed45955687b525e1f.png)
+ ⟶
Names
![oxygen + manganese ⟶ manganese monoxide](../image_source/b805ad5a8d3c9640db7c00b8683f0033.png)
oxygen + manganese ⟶ manganese monoxide
Reaction thermodynamics
Enthalpy
![| oxygen | manganese | manganese monoxide molecular enthalpy | 0 kJ/mol | 0 kJ/mol | -385.2 kJ/mol total enthalpy | 0 kJ/mol | 0 kJ/mol | -770.4 kJ/mol | H_initial = 0 kJ/mol | | H_final = -770.4 kJ/mol ΔH_rxn^0 | -770.4 kJ/mol - 0 kJ/mol = -770.4 kJ/mol (exothermic) | |](../image_source/593366d8e9685435aea95115f92c7eb1.png)
| oxygen | manganese | manganese monoxide molecular enthalpy | 0 kJ/mol | 0 kJ/mol | -385.2 kJ/mol total enthalpy | 0 kJ/mol | 0 kJ/mol | -770.4 kJ/mol | H_initial = 0 kJ/mol | | H_final = -770.4 kJ/mol ΔH_rxn^0 | -770.4 kJ/mol - 0 kJ/mol = -770.4 kJ/mol (exothermic) | |
Entropy
![| oxygen | manganese | manganese monoxide molecular entropy | 205 J/(mol K) | 32 J/(mol K) | 60 J/(mol K) total entropy | 205 J/(mol K) | 64 J/(mol K) | 120 J/(mol K) | S_initial = 269 J/(mol K) | | S_final = 120 J/(mol K) ΔS_rxn^0 | 120 J/(mol K) - 269 J/(mol K) = -149 J/(mol K) (exoentropic) | |](../image_source/341319134ce67fb37e92c2b133da031a.png)
| oxygen | manganese | manganese monoxide molecular entropy | 205 J/(mol K) | 32 J/(mol K) | 60 J/(mol K) total entropy | 205 J/(mol K) | 64 J/(mol K) | 120 J/(mol K) | S_initial = 269 J/(mol K) | | S_final = 120 J/(mol K) ΔS_rxn^0 | 120 J/(mol K) - 269 J/(mol K) = -149 J/(mol K) (exoentropic) | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: O_2 + Mn ⟶ MnO 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 Mn ⟶ 2 MnO 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 Mn | 2 | -2 MnO | 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) Mn | 2 | -2 | ([Mn])^(-2) MnO | 2 | 2 | ([MnO])^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) ([Mn])^(-2) ([MnO])^2 = ([MnO])^2/([O2] ([Mn])^2)](../image_source/2c22c6793672903d44336b9fd6cf556e.png)
Construct the equilibrium constant, K, expression for: O_2 + Mn ⟶ MnO 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 Mn ⟶ 2 MnO 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 Mn | 2 | -2 MnO | 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) Mn | 2 | -2 | ([Mn])^(-2) MnO | 2 | 2 | ([MnO])^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) ([Mn])^(-2) ([MnO])^2 = ([MnO])^2/([O2] ([Mn])^2)
Rate of reaction
![Construct the rate of reaction expression for: O_2 + Mn ⟶ MnO 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 Mn ⟶ 2 MnO 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 Mn | 2 | -2 MnO | 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) Mn | 2 | -2 | -1/2 (Δ[Mn])/(Δt) MnO | 2 | 2 | 1/2 (Δ[MnO])/(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[Mn])/(Δt) = 1/2 (Δ[MnO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/85bc105dab6a8c1877d48cedced47b85.png)
Construct the rate of reaction expression for: O_2 + Mn ⟶ MnO 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 Mn ⟶ 2 MnO 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 Mn | 2 | -2 MnO | 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) Mn | 2 | -2 | -1/2 (Δ[Mn])/(Δt) MnO | 2 | 2 | 1/2 (Δ[MnO])/(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[Mn])/(Δt) = 1/2 (Δ[MnO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| oxygen | manganese | manganese monoxide formula | O_2 | Mn | MnO name | oxygen | manganese | manganese monoxide IUPAC name | molecular oxygen | manganese | oxomanganese](../image_source/3eea838d6e2072de29076a3060583a98.png)
| oxygen | manganese | manganese monoxide formula | O_2 | Mn | MnO name | oxygen | manganese | manganese monoxide IUPAC name | molecular oxygen | manganese | oxomanganese
Substance properties
![| oxygen | manganese | manganese monoxide molar mass | 31.998 g/mol | 54.938044 g/mol | 70.937 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) melting point | -218 °C | 1244 °C | 1840 °C boiling point | -183 °C | 1962 °C | density | 0.001429 g/cm^3 (at 0 °C) | 7.3 g/cm^3 | 5.45 g/cm^3 solubility in water | | insoluble | insoluble surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | |](../image_source/24ca960b042b3462ce92ee2b20cd2f79.png)
| oxygen | manganese | manganese monoxide molar mass | 31.998 g/mol | 54.938044 g/mol | 70.937 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) melting point | -218 °C | 1244 °C | 1840 °C boiling point | -183 °C | 1962 °C | density | 0.001429 g/cm^3 (at 0 °C) | 7.3 g/cm^3 | 5.45 g/cm^3 solubility in water | | insoluble | insoluble surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | |
Units