I mix 8.15 grams of nitrogen, 3.76 grams of hydrogen and 4.19 grams of helium in a flask. If the total pressure in the system was found to be 301 kPa. How much pressure of the total does each gas exert? a) The pressure due to the hydrogen was Submit Answer Incorrect. Tries 7/99 Previous Tries b) The pressure due to the nitrogen was Tries 0/99 Submit Answer c) The pressure due to the helium was Submit Answer Tries 0/99
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
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![**Problem Statement:**
I mix 8.15 grams of nitrogen, 3.76 grams of hydrogen, and 4.19 grams of helium in a flask. If the total pressure in the system was found to be 301 kPa, how much pressure of the total does each gas exert?
**Questions:**
a) The pressure due to the hydrogen was _________
Submit Answer [Incorrect. Tries 7/99] [Previous Tries]
b) The pressure due to the nitrogen was _________
Submit Answer [Tries 0/99]
c) The pressure due to the helium was _________
Submit Answer [Tries 0/99]
**Instructions for Answering:**
- Provide the partial pressure of each gas individually by applying the principles of Dalton's Law of Partial Pressures and the Ideal Gas Law.
- Utilize the given mass of each gas to calculate moles, assuming you have access to their molar masses.
- Calculate each gas's contribution to the total pressure (301 kPa) based on its mole fraction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F05049175-dc72-4b68-b2f4-4f42a71730d2%2F91d5000f-a476-4ca2-aa2e-9f71a9d5772f%2Fa6bb9ku_processed.png&w=3840&q=75)
According to the kinetic molecular theory of gas, the pressure of a gas depends on the temperature, volume, and the number of moles of the gas and it does not depend on the nature of the gas.
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