Pressure remaining the same,the volume of a given mass of an ideal gas increases for every degree centigrade rise in temperature by a definite fraction of its volume at:

The correct gas equation is:

At $25 \, ^\circ C$,the density of oxygen gas is $1.458 \, mg/L$ at $1 \, atm$ pressure. What will be the pressure of oxygen gas if the density is doubled?

Consider the figure provided. $1 \ mol$ of an ideal gas is kept in a cylinder,fitted with a piston,at the position $A$,at $18^{\circ} C$. If the piston is moved to position $B$,keeping the temperature unchanged,then '$x$' $L \ atm$ work is done in this reversible process. $x=$ . . . . . . $L \ atm$. (nearest integer) [Given : Absolute temperature $=^{\circ} C + 273.15$,$R=0.08206 \ L \ atm \ mol^{-1} \ K^{-1}$]

At $N.T.P.$,the volume of a gas is found to be $273 \ mL$. What will be the volume of this gas at $600 \ mm \ Hg$ and $273 \ ^oC$? ................. $mL$

At $0^{\circ}C$,the density of a certain oxide of a gas at $2 \ bar$ is the same as that of dinitrogen at $5 \ bar$. What is the molecular mass of the oxide?