(II) A storage tank contains 21.6 kg of nitrogen (N2) at an absolute pressure of 3.85 atm. What

Name: Problem 36, Chapter 17: Physics for Scientists and Engineers with Modern Physics
Uploaded: 2019-06-20T07:23:12-08:00
Duration: 1 min 52 s
Channel: Sri Datta Vikas Buchemmavari
Description: (II) A storage tank contains 21.6 kg of nitrogen (N2) at an absolute pressure of 3.85 atm. What will the pressure be if the nitrogen is replaced by an equal mass of CO2 at the same temperature?

step 1 We have 21 .6 kilograms of nitrogen in a gas at 3 .85, uh, nitrogen gas in a fixed volume at 3 .

Question

(II) A storage tank contains 21.6 $\mathrm{kg}$ of nitrogen $\left(\mathrm{N}_{2}\right)$ at an absolute pressure of 3.85 atm. What will the pressure be if the nitrogen is replaced by an equal mass of $\mathrm{CO}_{2}$ at the same temperature?

   (II) A storage tank contains 21.6 $\mathrm{kg}$ of nitrogen $\left(\mathrm{N}_{2}\right)$ at an
absolute pressure of 3.85 atm. What will the pressure be if the nitrogen is replaced by an equal mass of $\mathrm{CO}_{2}$ at the same temperature?

Physics for Scientists and Engineers with Modern Physics

Douglas C. Giancoli 4th Edition

Chapter 17, Problem 36

Instant Answer

Solved by Expert Sri Datta Vikas Buchemmavari

06/20/2019

Step 1

According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. Since V and T are constant, we can say that P is directly proportional to n. Therefore, if we replace Show more…

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(II) A storage tank contains 21.6 $\mathrm{kg}$ of nitrogen $\left(\mathrm{N}_{2}\right)$ at an absolute pressure of 3.85 atm. What will the pressure be if the nitrogen is replaced by an equal mass of $\mathrm{CO}_{2}$ at the same temperature?

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Key Concepts

Ideal Gas Law

The ideal gas law (PV = nRT) is a fundamental relation that connects pressure, volume, temperature, and the number of moles of a gas. It explains that at constant volume and temperature, the pressure of a gas is directly proportional to the number of moles (n). This concept is essential when comparing changes in pressure due to the substitution of one gas for another under unchanged conditions.

Molar Mass and Mole Relationship

This concept involves understanding that the number of moles of a substance is calculated by dividing its given mass by its molar mass. Since different gases have different molar masses, the same mass of two different gases will contain different numbers of moles. This difference in mole numbers directly impacts the pressure of the gas in a fixed volume and constant temperature as described by the ideal gas law.

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