A sample of argon gas at stp occupies 56.2 liters. determine the number of moles of argon and the mass in the sample. for the above problem how will you rearrange the ideal gas law to solve for moles of argon?

we can use the ideal gas law equation to find the number of moles;
PV = nRT
where P - pressure
V - volume - 56.2 x 10⁻³ m³
n - number of moles
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature
standard temperature is 273 K
and standard pressure - 101 325 Pa
we can rearrange the equation to find the number of moles
[tex]n = \frac{PV}{RT} [/tex]
substituting the values in the equation
[tex]n = \frac{101325Pa*56.2 x 10⁻³ m³}{8.314 Jmol⁻¹K⁻¹*273K} [/tex]
n = 2.51 mol
molar mass of Ar - 40 g/mol
mass of Ar in the sample - 2.51 mol x 40 g/mol = 100.4 g

Eduard22sly Eduard22sly · Answer 2 · 2021-11-09T15:37:25+01:00

The number of mole and mass of argon are:

1. The number of mole of argon is 2.51 mole.

2. The mass of argon is 100.4 g

1. Determination of the number of mole of argon.

From the question given above, the following data were obtained:

Volume (V) = 56.2 L

Pressure (P) = stp = 1 atm

Temperature (T) = stp = 273 K

Gas constant (R) = 0.0821 atm.L/Kmol

Number of mole (n) =?

Using the ideal gas equation, the number of mole of argon can be obtained as follow:

PV = nRT

1 × 56.2 = n × 0.0821 × 273

56.2 = n × 22.4133

Divide both side by 22.4133

n = 56.2 / 22.4133

n = 2.51 mole

Therefore, the number of mole of argon is 2.51 mole

2. Determination of the mass of argon.

Mole of Ar = 2.51 mole

Molar mass of Ar = 40 g/mol

Mass of Ar =?

Mass = mole × molar mass

Mass of Ar = 2.51 × 40

Mass of Ar = 100.4 g

Thus, the mass of argon is 100.4 g

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