Question

17.
When 36.89 N,0.9) is introduced into a 1.0-litre flask at 27°C. The following equilibrium reaction
Occurs N.O.(9) 2N02 (g): k, = 0.1642 atm
(a) Calculate K of the equilibrium reaction.
(b) What are the number of moles of N2O, and NO2 at equilibriurn?
(c) What is the total gas pressure in the flask at equilibrium?
(d) What is the percent dissociation of N2O_?
07
100​

Answer 1

:-.ℕ

ℕ.=

.

⇒.

ℙ=ℝ

ℙ=

ℝ⇒

×

.

×.×=..

=

.−

()

=.

=.−.

+.−.==.

(a)K

C

=K

P

(RT)

−Δng

Δng=2−1=1

⇒0.1642×(0.084×300)

−1

⇒0.1642/24.63⇒0.0067