Respuesta :

Edufirst
Strategy: with the volume, pressure and temperature you can find the number of moles.

With the number of moles and the mass in grams you can find the molar mass of the gas, and with the molar mass you can figure out the gas.


1) pV = nRT => n = pV / RT

R = 0.082 atm*liter / mol*K
T = 62 + 273.15 = 335.15 K
p = 1.98 atm
V = 0.752 liter

n = (1.98 atm * 0.752 liter) / [0.082 atm* liter / (mol * K) * 335.15K] = 0.05418 mol


2) molar mass = mass / n = 2.49 g / 0.05418 mol = 45.96 g/mol ≈ 46.0 g/mol

So, now you must compare this molar mass with the molar masses of the list of choices.

For example, for NO2 the molar mass is 14 g/mol + 2 * 16 g/mol = 14 g/mol + 32 g/mol = 46 g / mol.

Given that NO2 is in the list of choices, you can conclude that the gas is NO2.
mahima6824soni

The volume of a sample of gas (2.49 g was 752 ml at 1.98 atm. and 62 °c. the gas is [tex]NO_2[/tex] ( nitrogen dioxide).

What is gas?

Gas is one of the states of matter. The gas does not have its shape and size. The particles of gas are far away from each other and move freely.

Now, if the temperature, pressure and volume are given we can find the number of moles.

With the moles we can find the molar mass and from the molar mass we can figure out the gas.

From the ideal gas law

PV = nRT

Temperature =62 °c  62+ 273.15 = (335.15 K)

Pressure =1.98 atm

Volume  =752 ml  (0.725 l)

R = 0.082 atm x liter / mol x K

Putting the values

[tex]\rm n = \dfrac{1.98 atm \times 0.752 liter}{0.082 atm\times liter / (mol \times K) \times 335.15K} \\\\n= 0.05418\; mol[/tex]

Calculating the molar mass

[tex]\begin{aligned} \rm Molar\;mass & = \dfrac{mass}{number\;of\;moles} }\\\\\rm Molar\;mass &= \dfrac{2.49\; g}{0.05418\; mol}\\\\&= 46.0 g/mol \end{aligned}[/tex]

The molar mass of [tex]NO_2[/tex] is 46.0 g.

Thus, the gas is [tex]NO_2[/tex].

Learn more about gas, here:

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