Question

There are three containers filled with different gases as shown.

Answer 1

$\qquad\qquad\huge\underline{{\sf Answer}}$

As we know,

$\sf \qquad density = \dfrac{mass}{volume}$

So, we can infer that :

$\sf \qquad mass= {density} \cdot{volume}$

Now, let's calculate the mass of gases in each case :

Case A : Hydrogen ~

$\qquad \sf \dashrightarrow \:mass = 0.09 \times (15) {}^{3}$

$\qquad \sf \dashrightarrow \:mass = 0.09 \times 3375 {}^{}$

$\qquad \sf \dashrightarrow \:mass = 303.75 \: \: mg {}^{}$

or

$\qquad \sf \dashrightarrow \:mass =0. 30375 \: \: g {}^{}$

Case B : Helium ~

$\qquad \sf \dashrightarrow \:mass =0. 175 \: \cdot \: (14 \sdot 12 \sdot10)$

$\qquad \sf \dashrightarrow \:mass =0. 175 \: \cdot \: 1680$

$\qquad \sf \dashrightarrow \:mass =0. 175 \: \cdot \: 294 \: \: mg$

or

$\qquad \sf \dashrightarrow \:mass = 0.294 \: \: g$

Case C : Nitrogen ~

$\qquad \sf \dashrightarrow \:mass = 1.251\: \cdot \: \dfrac{4}{3} \cdot3.14 \cdot(4) {}^{3}$

$\qquad \sf \dashrightarrow \:mass = 0.417\: \cdot \: 803.84$

$\qquad \sf \dashrightarrow \:mass = 335.201 \: \: mg$

or

$\qquad \sf \dashrightarrow \:mass = 0.335 \: \: g$

So, the arrangement of masses from least to greatest is :

• (1.) Hydrogen < (2.) Helium < (3.) Nitrogen