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 ...

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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

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0.26 g / L

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13 g / L

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26 g / L

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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
$\frac{2 \times 16}{0.082 \times 300} = 1.3 g / L$ .

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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 $C H_{4} = 16 g$ )