1 mole of H2 gas is contained in a box of volume V = 1.00 m3 at T = 300 K. The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

Question

1 mole of H2 gas is contained in a box of volume V = 1.00 m3 at T = 300 K. The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal) (A) same as the pressure initially (B) 2 times the pressure initially (C) 10 times the pressure initially (D) 20 times the pressure initially

Tardigrade Admin · Accepted Answer

According to gas equation PV = nRT or (P2V2/T2)=(P1V1/T1)or (P2/P1)=(V1/V2). (T2/T1) Here, T2 = 3000 K, T1 = 300 K Since H2 splits into hydrogen atoms, therefore volume become half i.e., V2=(1/2)V1 ∴ (P2 /P1)=(V1/(1)2V1)×(3000/300) or (P2/P1)=20

Q. 1mole of H2​ gas is contained in a box of volume V=1.00m3 at T=300K. The gas is heated to a temperature of T=3000K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

same as the pressure initially

2 times the pressure initially

10 times the pressure initially

20 times the pressure initially

Q. $1 m o l e$ of $H_{2}$ gas is contained in a box of volume $V = 1.00 m^{3}$ at $T = 300 K$ . The gas is heated to a temperature of $T = 3000 K$ and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)