Volume versus temperature graphs for a given mass of an ideal gas are shown in figure. At two different values of constant pressure. What can be inferred about relation between $p_1$ and $p_2$ ?

1 mole of $\mathrm{H}_2$ gas is contained in a box of volume $V=1.00 \mathrm{~m}^3$ at $T=300 \mathrm{~K}$. The gas is heated to a temperature of $T=3000 \mathrm{~K}$ and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

A vessel of volume $V$ contains a mixture of 1 mole of hydrogen and 1 mole oxygen (both considered as ideal). Let $f_1(v) d v$, denote the fraction of molecules with speed between $v$ and $(v+d v)$ with $f_2(v) d v$, similarly for oxygen. Then,

An inflated rubber balloon contains one mole of an ideal gas, has a pressure $p$, volume $V$ and temperature $T$. If the temperature rises to 1.1 T , and the volume is increased to 1.05 V , the final pressure will be

$A B C D E F G H$ is a hollow cube made of an insulator (figure) face $A B C D$ has positive charge on it. Inside the cube, we have ionised hydrogen. The usual kinetic theory expression for pressure