Question

One mole of CO2 occupies 1.5L at 250C Calculate the pressure exerted by gas using ideal gas equation​

Answer 1

Answer:

) 5 moles of CO

2

in 1l vessel of 47°C.

n=5,v=1l,t=273.15+47=320.15k

vanderwaal's equation of state, a=3.592

b=0.0427

(p+a

v

2

n

2

)(V−nb)=nrt

(p+3.592×

1

2

5

2

)(1−5×0.0427)=5×0.0821×320.15

(p+89.8)=167.1

Pressure,P=77.297atm

(b) Volume occupied by CO

2

gas is negligible (b=0).

vander waal's equation for 1 mole of gas is, (p+

v

2

a

)(v−b)=nrt⟶(i)

(p+

v

2

a

)(v)=nrt

P=

v

RT

−

v

2

a

Using R=0.0821,T=273K,v=22.4litre for 1 mole of an ideal gas.

P=

22.4

0.0821×273

−

22.4

2

3.592

=0.9934atm

Answer 2

Answer:

(a) By using the ideal gas law

P=

MV

WRT

=

44×0.5

22×0.0821×300

=24.63atm

(b) By using Van der Waals equation

P=

(V−nb)

nRT

−

V

2

an

2

=

0.5−(0.5×40×10

−3

)

0.5×0.0821×300

−

101.321×0.5

2

360×0.5

2

=25.66−3.55=22.1atom