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Argon gas has a temperature of 180°C at a pressure of 900 torr. If the gas is heated to 370°C, what is the new pressure of Argon gas in atmospheres (atm)? (Hint: 1 atm = 760 torr)

Sagot :

Lanuelidn

Based on the calculations, the final pressure of this gas sample at 370°C is equal to 2.66 atm..

Given the following data:

Initial temperature = 180°C.

Final temperature = 370°C.

Initial pressure = 900 torr.

Conversion:

760 torr = 1 atm.

900 torr = 1.29 atm.

How to determine the final pressure.

In order to calculate the final pressure of an ideal gas at constant volume, we would apply Gay Lussac's law.

Mathematically, Gay Lussac's law is given by this formula;

[tex]P\;\alpha \;T\\\\P=kT[/tex]

Where:

  • P is the pressure.
  • T is the temperature.
  • k is the constant of proportionality.

Substituting the given parameters into the formula, we have;

[tex]\frac{P_1}{T_1} =\frac{P_2}{T_2} \\\\\frac{1.29}{180} =\frac{P_2}{370} \\\\0.0072 =\frac{P_2}{370}\\\\P_2 = 0.0072 \times 370[/tex]

Final pressure = 2.66 atm.

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