Hello, Jay,
We can use the idela gas law, PV=nRT for this question. I'll use a value of 0.0821 L*atm/K*mol for the gas constant, R.
The choice for R is based on it's units - all are compatible with the data provided, except for temperature. We need to add 273.15 to convert C to K, Kelvin.
Rearrange to isolate the unknown, n, the moles of gas:
n = PV/RT
Enter the data and cross out units, where possible. We should be left with only moles.
n = (1 atm)(1212 L)/(0.0821 L^atm/K*mole)*(308.15 K)
n = 47.9 moles CO2
Bob
Robert S.
tutor
You are welcome, Jay. I have already answered the Everest question. Perhaps it wasn't posted when you wrote, but it's there now. 3270 liters, if I remember correctly.
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06/06/21
Jay G.
Thanks again appreciate it!
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06/06/21
Robert S.
tutor
You're welcome, again. I do make mistakes, so please let me know if you see something that doesn't make sense. The gas laws are primarily a challenge in keeping the units under control. Pressures alone: N/m^2, torr, bar, atm. Pa, kPa, and mmHg. Easy to make mistakes when falling asleep. What is standard pressure for each?
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06/06/21
Jay G.
Thank you! Very Helpful! Do you know how to do this one as well? At ocean level, or 101.3 kPa, 1212 L of CO2 enters the atmosphere. How many liters of CO2 would this be at the top of Mt. Everest, or 33 kPa?06/06/21