Consider this reaction occurring at 298 k:

n2o(g) + no2(g) ⇆ 3 no(g)

if a reaction mixture contains only n2o and no2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some no forms in the mixture.
what maximum partial pressure of no builds up before the reaction ceases to be spontaneous?

The question is incomplete, here is the complete question:

Consider this reaction occurring at 298 K:

If a reaction mixture contains only at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture.

What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous. Given that:

The maximum partial pressure of NO will be

Explanation:

For the given chemical equation:

The expression of for above equation follows:

When the reaction ceases to be spontaneous, the (at equilibrium)

Relation between standard Gibbs free energy and equilibrium constant follows:

where,

= Standard Gibbs free energy = 107.8 kJ/mol = 107800  J/mol  (Conversion factor: 1 kJ = 1000 J )

R = Gas constant =

T = temperature = 298 K

Putting values in above equation, we get:

Hence, the maximum partial pressure of NO will be

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in chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. the standard formula is c = m/v, where c is the concentration, m is the mass of the solute dissolved, and v is the total volume