Air contains 78.08% nitrogen, 20.095% oxygen, and 0.93% argon. A sample of air occupies 8 L at 273 K and applies a pressure of 2.45 atm to its container. The sample of air is heated to 550 K, at which time it takes up 11.8 L. What is the partial pressure of nitrogen after the air has been heated? A. 2.61 atm B. 261.57 atm C. 282.16 atm D. 1.91 atm

Option A is the correct option.

Explanation:

Partial pressure of N² :

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here we have to get the change of moles on decrease the volume of the reaction in gas phase.

the   per the given options it will decrease by (d) 11-50%

we know, on decreasing the volume of the gas phase reaction the reaction moves to the product side.

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:                   1 - α               α               α           = 1 + α

(concentration = moles/volume, as volume is 1 l)

(where α is the degree of dissociation)

now the dissociation constant in terms of concentration is :

=  

or,

or,   = (at v = 1l)

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:               (1 - α)/0.5           α/0.5         α/0.5       = (1 + α)/0.5

thus, the dissociation constant in terms of concentration is :

or,  

=  

so, the change of 1 : 1/0.5

or, 1: 2

thus it will decrease by 50%.

or, as per the given options it will decrease by 11-50%

it's c (engineer's do their work with mechanical stuff not on any living being)