Gaseous StateHard
Question
A vessel of volume 5 litre contains 1.4 g of nitrogen at a temperature 1800 K. The pressure of the gas if 30% of its molecules are dissociated into atoms at this temperature is :
Options
A.4.05 atm
B.2.025 atm
C.3.84 atm
D.1.92 atm
Solution
N2 → 2N
at t = 0
0
at t = tf
-x 2x
but, x = 30% of
Final number of mole =
- x + 2x = 
+ x = 
∴ P =
= 1.92 atm.
at t = 0
0at t = tf
-x 2xbut, x = 30% of
Final number of mole =
- x + 2x = + x = ∴ P =
= 1.92 atm.Create a free account to view solution
View Solution FreeMore Gaseous State Questions
A sample of a gas was heated from 30oC to 60oC at constant pressure. Which of the following statement(s) is/are true....The inversion temperature of hydrogen is (given van der Waal′s constants a and b are 0.244 atmL2mol-2 and 1.027 L ...A substance AxBy crystallizes in a face-centred cubic (fcc) Lattice in which atoms ′A′ occupy each corner of...Identify the correct statements when a fixed amount ideal gas is heated in from 300 to 600 K in a container fitted with ...Gaseous N2O4 dissociates into gaseous NO2 according to the reaction N2O4(g) ⇋ 2NO2(g) At 300 K and 1 atm pressure,...