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3 years ago

To what temperature must a 2.65 L container filled with 4.47 g of Ar be heated in order to obtain a pressure of 1.24 atm?

Chemistry

1 answer:

SVETLANKA909090 [29]3 years ago

8 0

The temperature of the container containing the 4.47 g of Ar is 358.16 K

<h3>How to determine the mole of Ar</h3>

Mass of Ar = 4.47 g
Molar mass of Ar = 40 g/mol
Mole of Ar =?

Mole = mass / molar mass

Mole of Ar = 4.47 / 40

Mole of Ar = 0.11175 mole

<h3>How to determine the temperature </h3>

Number of mole (n) = 0.11175 moles
Volume = 2.65 L
Pressure (P) = 1.24 atm
Gas constant (R) = 0.0821 atm.L/Kmol

Temperature (T) =?

The temperature of the container can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

Divide both side by nR

T = PV / nR

T = (1.24 × 2.65) / (0.11175 × 0.0821)

T = 358.16 K

Learn more about ideal gas equation:

brainly.com/question/4147359

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