Calculate density of CH 4 gas at the temperature 27- C and the pressure 2 bar Molecular mass of CH 4-16 g A- 1-3 g - LB- 0-26 g - LC- 13 g - LD- 26 g - L

The correct option is A 1.3 g/LWe know that, PV = nRT (ideal gas equation) PV = mMRT nbsp;(n = mM ) PV = mvRTM(mv = d ) P = dRTM where, pressure (P) n ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Dalton's Law of Partial Pressures

Calculate den...

Question

Calculate density of $C H_{4}$ gas at the temperature $27^{\circ} C$ and the pressure 2 bar (Molecular mass of $C H_{4} = 16 g$ )

1.3 g / L

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

0.26 g / L

No worries! We‘ve got your back. Try BYJU‘S free classes today!

13 g / L

No worries! We‘ve got your back. Try BYJU‘S free classes today!

26 g / L

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $1.3 g / L$
We know that,
$P V = n R T$ (ideal gas equation)
$P V = \frac{m}{M} R T (n = \frac{m}{M}) P V = \frac{m}{v} \frac{R T}{M} (\frac{m}{v} = d) P = \frac{d R T}{M}$
where,
pressure (P) = 2 bar , density (d)= ?
T = temperature $= 27 + 273 = 300 K$
R = gas constant = $0.082 L a t m m o l^{- 1} K^{- 1}$
M = 16 g
Substituting the values in the formula
$\frac{2 \times 16}{0.082 \times 300} = 1.3 g / L$ .

Suggest Corrections

Similar questions

The density of a gas is 2 $\frac{g}{L}$ at 1 atm and $27^{0} C$ . The density of the same gas at 2 atm and $127^{0} C$ is:

Q. At

273 K

temperature and

76 c m H g

pressure, the density of a gas is

1.964 g L^{- 1} .

The gas is :

Q. At a definite temperature, rate of diffusion of

C H_{4}

gas is twice that of gas X, then calculate molecular mass of X?

Q. If the density of a gas at

27^{0}

C

and 1 atmospheric pressure is

1.8

(

g / L

) ,its molecular mass is :

Q. What is the density of wet air ( in g/L) which have a partial pressure of water of 22.5 torr at 1 atm and

300 K

(

Given: vapour pressure of

H_{2} O

is 30 torr and the average molar mass of air is

29 g)

Join BYJU'S Learning Program

Calculate density of CH4 gas at the temperature 27∘C and the pressure 2 bar (Molecular mass of CH4=16 g)

The correct option is A 1.3 g/LWe know that, PV=nRT (ideal gas equation) PV=mMRT(n=mM)PV=mvRTM(mv=d)P=dRTM where, pressure (P) = 2 bar , density (d)= ? T = temperature =27+273=300K R = gas constant =0.082 L atm mol−1 K−1 M = 16 g Substituting the values in the formula 2×160.082×300=1.3 g/L.

Calculate density of $C H_{4}$ gas at the temperature $27^{\circ} C$ and the pressure 2 bar (Molecular mass of $C H_{4} = 16 g$ )