Question

The density of O3 gas which has
Pressure 730 mm of Hg at 50 c is​

Answer 1

Explanation:

P=730mm

V=380mL

P

′

=760mm

V

′

=?

At constant temperature,

PV=P

′

V

′

730mm×380mL=760mm×V

′

V

′

=365mL

Hence, the volume occupied by the oxygen at 760 mm pressure is 365 mL.

Answer 2

Answer:

The density of $O_{3}$ gas is 2.201 g/L.

Explanation:

As per the data given in the question

we have to calculate The density of $O{3}$ gas

As per the questions

It is given that

Pressure 730 mm of Hg at 50°c

As we know in Ideal gas equation PV=nRT

⇒P=$\frac{nRT}{V}$

⇒P=$\frac{\frac{w}{m}RT }{V}$

we know density =mass/volume

so, P=$\frac{d*R*T}{m}$

As per question

pressure=730mm

1 atm=760mm of Hg

so pressure=$\frac{730}{760}$ =0.96 atm

now we convert degree Celsius to kelvin.

T=50+273=323 K

As we know in atmospheric pressure the value of R=0.081 liter atm $K^{-1}$$mol^{-1}$

Molar mass of $Co_{3}$ is =(molar mass of carbon+ 3*molar mass of oxygen)

Molar mass of $Co_{3}$ is=12+48=60 g/mol

Applying formula P=$\frac{d*R*T}{m}$.

⇒d=$\frac{60*0.96}{0.081*323}$

⇒$\frac{57.6}{26.163}$

⇒d=2.201$\frac{g}{L}$

Hence, the density of $O_{3}$ gas is 2.201 g/L.

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