Question

A vessel with a volume of 25.1 L contains 2.80 g of nitrogen gas, 0.605 g of hydrogen gas, and 79.9 g of argon gas. At
25°C, what is the pressure in the vessel?
Select one:
a. 58.7 atm
b. 2.73 atm
c. 0.196 atm
d. 81.0 atm
e. 2.34 atm

Answer 1

2.73 atm is the pressure in the vessel. Hence, option B is correct.

What is an ideal gas equation?

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= ?

V= 25.1 L

$n= \frac{m}{molar \;mass \;of \;nitrogen} + \frac{m}{molar \;mass \;of \;hydrogen } +\frac{m}{molar \;mass \;of \;argon}$

$n= \frac{2.80 g}{14} + \frac{0.605 g}{1} +\frac{79.9 g}{40}$

n= 2.8025

R= $0.082057338 \;L \;atm \;K^{-1}mol^{-1}$

T=25°C + 273= 298 K

Putting value in the given equation:

$\frac{PV}{RT}=n$

$2.8025 = \frac{P\; X \;25.1 \;L}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 298}$

P = 2.73 atm

2.73 atm is the pressure in the vessel. Hence, option B is correct.

Learn more about the ideal gas here:

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