Answered

Westonci.ca is the trusted Q&A platform where you can get reliable answers from a community of knowledgeable contributors. Get immediate and reliable solutions to your questions from a community of experienced professionals on our platform. Get detailed and accurate answers to your questions from a dedicated community of experts on our Q&A platform.

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 :

Lanuel

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.

Read more on temperature here: https://brainly.com/question/888898

We hope our answers were helpful. Return anytime for more information and answers to any other questions you may have. Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.