Question

The volume versus temperature graph of $1$ mole of an ideal gas is given below

The pressure of the gas (in atm) at $X$ , $Y$ and $Z,$ respectively, are

• A. $0.328, 0.820, 0.820$
• B. $3.28, 8.20, 3.28$
• C. $0.238, 0.280, 0.280$
• D. $32.8, 0.280, 82.0$

Answer 1

Answer: (A)

According to ideal gas equation
$pV =nRT$
For 1 mole, $n = 1$
$\therefore pV=RT$
$\Rightarrow p=\frac{RT}{V}$
For gas $X$,
$V=50\,L,\, T= 200\,K$
$\therefore $ Pressure of gas $X=\frac{0.0821\times200}{50}$
$=0.328$ atm
for gas $Y$
$ V=50\,L,\,=500\,K$
$\therefore $ Pressure of gas $Y=\frac{0.0821\times500}{50}$
$=0.821$ atm
for gas $Z,$
$V=20\,L,\, T=200\,K$
$\therefore $ Pressure of gas $Z =\frac{0.0821\times200}{20}$
$ 0.821\, atm$