Question

Q46) The density (in g/L) of CH4 gas present in 1 litrevessel at 15 atm and 400 K is [R = 0.8 atm-L/mol K]​

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Answer 1

Answer:

The density (in g/L) of CH4 gas present in 1 litrevessel at 15 atm and 400 K is [R = 0.8 atm-L/mol K] - 21813242.

Answer 2

Given:

CH4 gas present in 1-litre vessel at 15 atm and 400 K

To find:

The density

Solution:

To solve the given-problem we will use the Ideal Gas Law which is as follows:

$\boxed{\bold{PV = nRT}}$

Here we have,

Volume, V = 1 litre

Pressure, P = 15 atm

Temperature, T = 400 K

Ideal gas constant, R = 0.8 atm-L/mol K

No. of moles, n = $\frac{Mass}{Molar \:mass}$

The molar mass of CH₄ = 12 + (1 × 4) = 16 g/mol

Let "m" grams represent the mass of CH₄ gas.

On substituting the given values in the ideal gas law expression, we get

$15 \times 1 = \frac{m}{16} \times 0.8 \times 400$

$\implies 15 \times 16 = m \times 0.8 \times 400$

$\implies 240 = m \times 320$

$\implies m = \frac{240}{320}$

$\implies \bold{m = 0.75\:gm}$

Now,

The density of CH₄ in gm/L is,

= $\frac{Mass}{Volume}$

= $\frac{0.75\:gm}{1 \:litre}$

= $\bold{0.75\:g/L}$

Thus, the density (in g/L) of CH4 gas present in 1 litre vessel at 15 atm and 400 K is → 0.75 g/L.

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