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lys-0071 [83]
3 years ago
5

A flask at room temperature contains exactly equal amounts (moles of nitrogen and oxygen.

Chemistry
1 answer:
brilliants [131]3 years ago
7 0
<span>Equal amounts (moles of nitrogen and oxygen).

a. which gas has the higher partial pressure?

Partial pressure is proportional to the molar fraction of the gas.

Given that there are equal amounts, the molar fractions and the partial pressures are equal.

b. molecules of which gas have the higher average velocity?

The average velocity is inversely related to the square root of molar mass of the gas, then the gass with the lower molar mass will have the higher average velocity.

Molar mass of N2 = 2 * 14 g/mol = 28 g/mol
Molar mass of O2 = 2 * 16 g/mol = 32 g/mol

Then, N2 will have a higher average velocity.


c. the molecules of which gas effuses more quickly if a small hole was opened in the flask?

The effusion rate is inversely related to the square root of the molar mass, then the gas with the lower molar mass will effuse more quickly.

Therefore, N2 will effuse more quickly.
</span>
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A 0.223 mole sample of gas is held at 33.0 C and 2.00 atm, What's the volume of the gas? R = 0.0821 L atm / mol K answer soon il
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Answer:

The volume of the gas is 2.80 L.

Explanation:

An ideal gas is a theoretical gas that is considered to be made up of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The Pressure (P) of a gas on the walls of the container that contains it, the Volume (V) it occupies, the Temperature (T) at which it is located and the amount of substance it contains (number of moles, n) are related from the equation known as Equation of State of Ideal Gases:

P*V = n*R*T

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In this case:

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Replacing:

2 atm* V= 0.223 moles*0.0821 \frac{L*atm}{mol*K}* 306 K

Solving:

V=\frac{0.223 moles*0.0821\frac{L*atm}{mol*K} * 306 K}{2 atm} \\

V= 2.80 L

<u><em>The volume of the gas is 2.80 L.</em></u>

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