Question

what is the molar value of N2 at 700k and 600 atm according to (a) ideal gas law b) virial equation . the virial equation B of N2 At 500 k = 0.0169 L/ mol.?

Answer 1

The virial equation of state reads:

Z=1+(b−aRT)1Vm+(bVm)2⋯Z=1+(b−aRT)1Vm+(bVm)2⋯

Going by this equation, it seems like increasing the value of bb will increase ZZ, which means repulsive forces will increase, making the gas liquefaction difficult. Also for a=0a=0 and b=0b=0, the gas becomes an ideal gas whose liquefaction is not possible, so I think what you are saying is incorrect.

The question you are talking about, that why chlorine is more easily liquefied than ethane? It is because aaof Cl2ClX2 is greater than aa of C2H6CX2HX6, which means Cl2ClX2 is easier to liquify. C2H6CX2HX6, being greater in size than Cl2ClX2, has a higher value of bb. It's wrong to say "the smaller the value of bb, the larger the liquefaction".

Answer 2

ANSWERS :-


$here \: is \: your \: solution \:$

(a) For 1 mole of an ideal gas ,

V = RT/P

= 0.0821 * 500/600

= 6.84 * 10^–2 L/mol

(b). using virial equation, Neglecting higher powers

Z = PV/RT

= 1 + B/V

= 1 + BP/RT

=>Z = 1 + 0.0169 * 600/0.0821 * 500

Z = 1.247

$for \: 1 \: mole \: real \: gas$

V = ZRT/P

= 1.247 * 0.0821 * 500/600

= 8.53 * 10^–2 L mol^-1


__________________________________

❤BE BRAINLY ❤
-----------------------------
------------------------------