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

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.