One mole of N2O4 gas at 300 K is kept in a closed container at 1 atm. It is heated to 600 K when 20 percent by mass of N2O4 decomposes to NO2(g). The resultant pressure in the container would be

Question

One mole of N2O4 gas at 300 K is kept in a closed container at 1 atm. It is heated to 600 K when 20 percent by mass of N2O4 decomposes to NO2(g). The resultant pressure in the container would be (A) 1.2 atm (B) 2.4 atm (C) 2 .0 atm (D) 1.0 atm

Tardigrade Admin · Accepted Answer

N2O4----->2 NO2 Initial 1 mol Ateqm. (1-0.2)mol 0.4 mol =0.8 mol Total moles after dissociation, n2=0-8+0-4= 1.2 Initial temperature = 300 K P1 V = n1 RT1 or 1 × V = 1 × R × 300 ...(i) Temperature after dissociation = 600 K. No. of moles after dissociation, n2 = 12 P2 × V = 1.2 × R × 600 ...(ii) Dividing eqn. (ii) by eqn. (i) p2=(1.2× 600/300)=2.4 atm

Q. One mole of N2​O4​ gas at 300 K is kept in a closed container at 1 atm. It is heated to 600 K when 20 percent by mass of N2​O4​ decomposes to NO2​(g). The resultant pressure in the container would be

1.2 atm

2.4 atm

2 .0 atm

1.0 atm

Q. One mole of $N_{2} O_{4}$ gas at 300 K is kept in a closed container at 1 atm. It is heated to 600 K when 20 percent by mass of $N_{2} O_{4}$ decomposes to $N O_{2} (g)$ . The resultant pressure in the container would be