Question

A flask of 8.21 litre contains CH4 gas at a pressure of 2 atm. Find moles of CH4 gas at 400k

Answer 1

Explanation:

using ideal gas equation

pv=nRT

n=pv/RT

using above data we get,

n= 2×8.21/0.0821×400

N=0.5 mol

Answer 2

Answer:

The number of moles of CH₄ gas at 400k is 0.5.

Explanation:

• We will use the ideal gas equation to solve this question. Which is given as,

                                                     $\mathrm{PV=nRT}$          (1)

Where,

P=pressure at which the gas is present

V=volume occupied by the gas

n=number of moles of the gas

R=universal gas constant= 0.0821 L.atm.K⁻¹.mol⁻¹

T=temperature in kelvin

From the question, we have the following condition at which CH₄ gas is present,

The pressure at which the gas is present(P)=2 atm

The volume occupied by the gas(V)=8.21 liter

The temperature at which the gas is present(T)=400K

By inserting all the values in equation (1) we get;

$\mathrm{2\times 8.21=n\times 0.0821\times 400}$

$\mathrm{n=\frac{2\times 8.21}{0.0821\times 400} }$

$\mathrm{n=\frac{1}{2} }$

$\mathrm{n=0.5}$

Hence, the number of moles of CH₄ gas at 400k is 0.5.

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