Boyles temperature (T $_{B}$ ) of CO $_{2}$ = 350C, T $_{B}$ of H $_{2}$ = 150C, T $_{B}$ of CH $_{4}$ = 60C

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Solution

(A) CO $_{2}$ gas at low pressure and at temp 573K obeys the idela gas law PV $=$ nRT.
It is more compressible than that of ideal gas.
It can not be liquified at any pressure.
Its Molar volume is lower than that of ideal<br><br>gas at same pressure and temperature.
(B) H $_{2}$ gas at (P~0, 273K) is more compressible than that of ideal gas.
(C) CO $_{2}$ gas in very high pressure region & temperature 623 K.
It can not be liquefied at any pressure.
(D) CH $_{4}$ gas at 333K & in low pressure region is more compressible than that of ideal gas.

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Assuming $C O_{2}$ to be van der waals gas, calculate its Boyle temperature. Given $a = 3.59 a t m L^{2} m o l^{- 2} b = 0.0427 L m o l^{- 1}$

Boyle temperature $T_{b}$ is

x = a \sin 2 t (1 + \cos 2 t) and y = b \cos 2 t (1 - \cos 2 t)

t = \frac{π}{4}, \frac{d y}{d x} = \frac{b}{a}

t = \frac{π}{4}, \frac{d y}{d x} = \frac{b}{a}

\sqrt{5}

T

t^{\circ} C

R_{t} = R_{0} (1 + a t + b t^{2})

R_{0}

0^{\circ} C .

t^{\circ} C

Δ H

Δ E

C H_{4 (g)} + 2 O_{2 (g)} ⇌ C O_{2 (g)} + 2 H_{2} O_{(l)}

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