1. To experiment with gas pressure and the ideal gas law, a student uses an open- ended manometer with a 7.2 L container for holding gas. The student then adds G.H g of methane gas (CH4) to the container at 10 °C. If atmospheric pressure is 107 kPa, (G and H are the last 2 digits of you ID number) A. Calculate how high the mercury will rise (mm) and in which direction (towards the gas or atmosphere), and draw a picture of the manometer with the CH4 gas inside. Assume ideal conditions. B. Describe two things you could do to the gas to make the liquid mercury levels equal (Ah = 0)? For each answer give an atomic-scale explanation of how that method will even out the mercury levels. 2. An unknown gas is found to have a density of G.H g/L. When the temperature is 79.1 °C, the pressure of the gas is 1.45 atm. What is the molar mass of the gas?
1. To experiment with gas pressure and the ideal gas law, a student uses an open- ended manometer with a 7.2 L container for holding gas. The student then adds G.H g of methane gas (CH4) to the container at 10 °C. If atmospheric pressure is 107 kPa, (G and H are the last 2 digits of you ID number) A. Calculate how high the mercury will rise (mm) and in which direction (towards the gas or atmosphere), and draw a picture of the manometer with the CH4 gas inside. Assume ideal conditions. B. Describe two things you could do to the gas to make the liquid mercury levels equal (Ah = 0)? For each answer give an atomic-scale explanation of how that method will even out the mercury levels. 2. An unknown gas is found to have a density of G.H g/L. When the temperature is 79.1 °C, the pressure of the gas is 1.45 atm. What is the molar mass of the gas?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.128QP: Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do...
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G.H= 7.2< please help this work..
![1.
To experiment with gas pressure and the ideal gas law, a student uses an open-
ended manometer with a 7.2 L container for holding gas. The student then adds G.H g of methane gas (CH4) to
the container at 10 °C. If atmospheric pressure is 107 kPa, (G and H are the last 2 digits of you ID number)
A. Calculate how high the mercury will rise (mm) and in which direction (towards the gas or atmosphere),
and draw a picture of the manometer with the CH4 gas inside. Assume ideal conditions.
B. Describe two things you could do to the gas to make the liquid mereury levels equal (Ah = 0)? For each
answer give an atomic-scale explanation of how that method will even out the mercury levels.
2.
An unknown gas is found to have a density of G.H g/L. When the temperature is 79.1 °C, the
pressure of the gas is 1.45 atm. What is the molar mass of the gas?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7ae764b7-d237-4053-a9e9-5b016ede3169%2Ffe793f32-f1e8-409c-9a51-7b5f0ffd5a4e%2F1f1h2qk_processed.png&w=3840&q=75)
Transcribed Image Text:1.
To experiment with gas pressure and the ideal gas law, a student uses an open-
ended manometer with a 7.2 L container for holding gas. The student then adds G.H g of methane gas (CH4) to
the container at 10 °C. If atmospheric pressure is 107 kPa, (G and H are the last 2 digits of you ID number)
A. Calculate how high the mercury will rise (mm) and in which direction (towards the gas or atmosphere),
and draw a picture of the manometer with the CH4 gas inside. Assume ideal conditions.
B. Describe two things you could do to the gas to make the liquid mereury levels equal (Ah = 0)? For each
answer give an atomic-scale explanation of how that method will even out the mercury levels.
2.
An unknown gas is found to have a density of G.H g/L. When the temperature is 79.1 °C, the
pressure of the gas is 1.45 atm. What is the molar mass of the gas?
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