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?

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Chapter1: Chemical Foundations
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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?
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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