You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Heat Capacity at Constant Pressure

One mole of ...

Question

One mole of $N_{2} O_{4} (g)$ at $300$ K is kept in a closed container under 1 atm. It is heated to $600$ K when 20% by mass of $N_{2} O (g)$ decomposes to $N O_{2} (g)$ .
The resultant pressure is :

1.2

atm

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2.5

atm

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

2.0

atm

No worries! We‘ve got your back. Try BYJU‘S free classes today!

1.0

atm

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C $2.5$ atm
$N_{2} O_{4} 1 (1 - 0.2) ⇌ 2 N O_{2} 0 2 \times 0.2 = 0.4$

Total pressure $= 1.2$

As the temperature is doubled, the pressure becomes double. Therefore, the total final pressure is.
$1.2 \times 2 = 2.4 a t m$ .

Suggest Corrections

Similar questions

Q. One mole of

N_{2} O_{4} (g)

at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of

N_{2} O (g)

decomposes to

N O_{2} (g) .

The resultant pressure is

Q. One mole of

N_{2} O_{4} (g)

300 K

and

1.0 a t m

is kept in a closed container. It is heated to

600 K

when

20 %

by mass of

N_{2} O_{4} (g)

decomposes to

N O_{2} (g)

. The resultant pressure is:

Q. One mole of

N_{2} O_{4} (g)

300 K

and

1.0 a t m

is kept in a closed container. It is heated to

600 K

when

20 %

by mass of

N_{2} O_{4} (g)

decomposes to

N O_{2} (g)

. The resultant pressure is:

Q. 1 mole of

N_{2} O_{4} (g)

at 300K is kept in a closed container under 1 atm pressure. It is heated to 600K when 20

%

by mass of

N_{2} O_{4} (g)

decomposes to

N O_{2} (g)

. The resultant pressure is

Q. One mole of

N_{2} O_{5} (g)

at 300 K is left in a closed container under one atm. It is heated to 600 K when 20% by mass of

N_{2} O_{5} (g)

decomposes to

N O_{2} (g)

. The resultant pressure is:

Join BYJU'S Learning Program

One mole of N2O4(g) at 300 K is kept in a closed container under 1 atm. It is heated to 600 K when 20% by mass of N2O(g) decomposes to NO2(g). The resultant pressure is :

The correct option is C 2.5 atmN2O41(1−0.2)⇌2NO202×0.2=0.4Total pressure =1.2As the temperature is doubled, the pressure becomes double. Therefore, the total final pressure is.1.2×2=2.4 atm.

One mole of $N_{2} O_{4} (g)$ at $300$ K is kept in a closed container under 1 atm. It is heated to $600$ K when 20% by mass of $N_{2} O (g)$ decomposes to $N O_{2} (g)$ .
The resultant pressure is :

The correct option is C $2.5$ atm
$N_{2} O_{4} 1 (1 - 0.2) ⇌ 2 N O_{2} 0 2 \times 0.2 = 0.4$

Total pressure $= 1.2$

As the temperature is doubled, the pressure becomes double. Therefore, the total final pressure is.
$1.2 \times 2 = 2.4 a t m$ .