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

particle   p is an electron and particle q is a neutron

question: ray weighs 100 kilograms, his wrestling partner, bobby, weighs 50 kilograms. if ray moves at 4 m s , how fast will bobby have to run at him to apply an equal amount of kinetic energy?

answer: 8 m/s he needs to run twice as fast to keep up so he has some work to do

explanation:   if the mass has units of kilograms and the velocity of meters per second, the kinetic energy has units of kilograms-meters squared per second squared.

question answered by

(jacemorris04)