Q1: At standard conditions,
N₂ + 2O₂  2NO₂; ΔG° = 100 kJ/mole
NO + O₂  2NO₂; ΔG° = -35 kJ/mole
The standard free energy of formation of NO in kJ/mole is

ANS:C - 85

To find the standard free energy of formation (Δ𝐺𝑓∘ΔGf∘​) of NO (nitric oxidenitric oxide), we can use the concept of Hess's law, which states that the total enthalpy change of a reaction is independent of the pathway taken. We have the following reactions:

1. 𝑁2+2𝑂2→2𝑁𝑂2N2​+2O2​→2NO2​; Δ𝐺∘=100 kJ/molΔG∘=100kJ/mol
2. 𝑁𝑂+𝑂2→2𝑁𝑂2NO+O2​→2NO2​; Δ𝐺∘=−35 kJ/molΔG∘=−35kJ/mol

We want to find the Δ𝐺𝑓∘ΔGf∘​ of 𝑁𝑂NO, which is the standard free energy change for the formation of 𝑁𝑂NO from its constituent elements in their standard states. We can manipulate the given equations to find the desired reaction, which is the formation of 𝑁𝑂NO:

1. Reverse equation 2: 2𝑁𝑂2→𝑁𝑂+𝑂22NO2​→NO+O2​; Δ𝐺∘=35 kJ/molΔG∘=35kJ/mol
2. Reverse equation 1 and multiply by 2: 2𝑁𝑂2→𝑁2+2𝑂22NO2​→N2​+2O2​; Δ𝐺∘=−200 kJ/molΔG∘=−200kJ/mol

Now, we can add these two equations together to get the desired reaction: 2𝑁𝑂2+2𝑁𝑂2→𝑁2+2𝑂2+𝑁𝑂+𝑂22NO2​+2NO2​→N2​+2O2​+NO+O2​ This simplifies to: 4𝑁𝑂2→𝑁2+3𝑂2+𝑁𝑂4NO2​→N2​+3O2​+NO And the Δ𝐺∘ΔG∘ for this reaction is 35 kJ/mol−200 kJ/mol=−165 kJ/mol35kJ/mol−200kJ/mol=−165kJ/mol The standard free energy of formation (Δ𝐺𝑓∘ΔGf∘​) of 𝑁𝑂NO can be calculated using this reaction: Δ𝐺𝑓∘(𝑁𝑂)=−Δ𝐺∘ΔGf∘​(NO)=−ΔG∘ Δ𝐺𝑓∘(𝑁𝑂)=−(−165 kJ/mol)ΔGf∘​(NO)=−(−165kJ/mol) Δ𝐺𝑓∘(𝑁𝑂)=165 kJ/molΔGf∘​(NO)=165kJ/mol So, the standard free energy of formation of 𝑁𝑂NO in kJ/mol is 165165 kJ/mol. Therefore, none of the provided options is correct.