How Does Temperature Affect NO2 Formation in Combustion?

[Dynamic24]

Homework Statement

We discussed the fact that the formation of some trace gases is thermodynamically unfavorable at low temperature, but more favorable at elevated temperatures. Using the values for delta G and delta H in the notes, calculate the equilibrium partial pressure of NO2 during combustion at at 1 atm and T = 1600 K.

The Attempt at a Solution

Just getting stuck on what the partial pressure of [N] and [O2] are.

 

[Borek]

Calculate K for the reaction, assume you start with just NO₂, then pressures of other gasses can be calculated from the reaction stoichiometry.

The wording seems to be unclear.

--

 

[Blueshift5]

I would first clarify the context and assumptions of this question. Is this a theoretical calculation or an experimental measurement? Are we assuming ideal gas behavior or accounting for any deviations? Are there any other reactants or products involved in the combustion process?

Once these details are established, I would proceed with the calculation by using the given values for delta G and delta H to determine the equilibrium constant (K) for the reaction of interest. Then, using the ideal gas law and the molar ratios of the reactants and products, I would calculate the partial pressures of [N] and [O2] at 1 atm and 1600 K. Finally, I would plug these values into the expression for the equilibrium constant to solve for the partial pressure of NO2.

It is also important to consider the potential impact of temperature and pressure on the combustion process and the resulting partial pressures. If the conditions of 1 atm and 1600 K are not realistic or relevant, it may be necessary to adjust the calculation accordingly. Additionally, it may be beneficial to compare the calculated partial pressure of NO2 to experimental data or other theoretical models to validate the results.