The decomposition of dinitrogen tetraoxide (N2O4) into nitrogen gas (N2) and oxygen gas (O2) is shown by which balanced chemical equation? a. N2O4 → N2 + O2
b. N2 + 2O2 → N2O4This answer is incorrect.
c. N2O4 → N2 + 2O2
d. N2O4 + 2O2 → N2

C. N₂O₄ → N₂ + 2O₂

General Formulas and Concepts:

Chemistry - Reactions

Explanation:

Step 1: Define

N₂O₄ decomposes into N₂ and O₂

Step 2: RxN

Unbalanced RxN:   N₂O₄ → N₂ + O₂

Balanced RxN:   N₂O₄ → N₂ + 2O₂

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%

for points guys