Nuts & Volts
Nuts & Volts
Nuts & Volts
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ties can drop to only a few meters and<br />
the dirt will sandblast astronaut’s<br />
visors. So to safely launch a balloon<br />
during a dust storm, astronauts will<br />
have to fill the balloon inside of a<br />
structure, like a shed. After they finish<br />
filling the balloon, they’ll carry it<br />
outside and release it. This is the same<br />
way the National Weather Service fills<br />
and launches their radiosondes.<br />
The Mars Pathfinder, which<br />
landed on Mars in July 1997, carried a<br />
set of wind socks on its ASI/MET<br />
mast. Pathfinder’s windsock data<br />
indicated that the Martian winds are<br />
at their strongest from morning to<br />
noon and weakest in the late<br />
afternoon and early evening.<br />
So it appears astronauts can fill<br />
and launch weather balloons on Mars.<br />
It will be easier if they wait until after<br />
noon local time to fill the balloon. But<br />
if they want to launch during a dust<br />
storm, they’ll need to use a filling shed.<br />
THE COMPOSITION<br />
OF THE MARTIAN<br />
ATMOSPHERE<br />
Let’s assume our astronauts want<br />
to launch a four pound (1,816 grams)<br />
payload and 6.6 pound (3,000 grams)<br />
weather balloon. Mars has a surface<br />
gravity that’s 38% of Earth’s gravity.<br />
Therefore, on Mars, the payload will<br />
only weigh 1.5 pounds and the balloon<br />
2.5 pounds. For our weather balloon to<br />
launch this payload, it must contain<br />
enough helium to displace at least four<br />
pounds of Martian atmosphere (the<br />
weight of the payload and balloon).<br />
Because gravity affects the weight<br />
of air and the payload alike, we won’t<br />
calculate weights on Mars, but just<br />
use mass. So in this case, the balloon<br />
must displace an atmospheric mass<br />
of at least 4,812 grams before the<br />
balloon can begin lifting the payload.<br />
An Avogadro’s number of gas molecules<br />
at standard temperature and<br />
pressure (STP) occupies a volume of<br />
22.4 liters and has a mass that is equal<br />
to the gas’ atomic weight. Did you get<br />
all of that I guess I should explain a<br />
few things about that sentence.<br />
Avogadro’s number is 6.022 x 10 23<br />
and it’s the number of molecules in one<br />
mole of any chemical. One mole of a<br />
chemical is an amount of that chemical<br />
that has a weight in grams that’s equal<br />
to its atomic mass. So one mole of<br />
hydrogen gas weighs two grams, occupies<br />
a volume of 22.4 liters at STP, and<br />
contains 6.022 x 10 23 molecules<br />
(remember that hydrogen gas is diatomic,<br />
or contains two hydrogen atoms).<br />
Standard temperature and pressure<br />
is a temperature of 0 degrees C<br />
(or 273 Kelvins) and a pressure of one<br />
atmosphere (1,013 mb). A Kelvin is<br />
equal to a degree Celsius. The only<br />
difference between them is that the<br />
Kelvin temperature scale begins at<br />
-273 degrees Celsius, or the temperature<br />
of absolute zero, while the<br />
Celsius scale begins at the freezing<br />
point of pure water. The Kelvin temperature<br />
scale doesn’t use the word<br />
“degrees” like Fahrenheit or Celsius.<br />
So please say the temperature is 273<br />
Kelvins and not 273 degrees Kelvin.<br />
The Martian atmosphere is 95%<br />
CO 2 , 3% N 2 , and 2% is trace gases.<br />
We’ll treat the Martian atmosphere as<br />
if it were pure carbon dioxide since<br />
the nitrogen and other trace gases<br />
only affect the density of the Martian<br />
atmosphere by a small amount. Since<br />
the chemical formula of carbon dioxide<br />
is CO 2 , its atomic mass is equal to<br />
the atomic mass of one carbon atom<br />
plus two oxygen atoms. By ignoring<br />
isotopes, I calculate the mass of a carbon<br />
dioxide molecule to be (1 x 12) +<br />
(2 x 16), or 44 atomic mass units.<br />
So an atmosphere of pure carbon<br />
dioxide has a mass of 44 grams per<br />
22.4 liters at STP. Helium has a mass<br />
of four grams per 22.4 liters at STP, so<br />
22.4 liters of helium will displace 40<br />
grams of carbon dioxide at STP.<br />
However, the air temperature at the<br />
Martian surface is -14 degrees C (259<br />
K) and the pressure is seven millibars.<br />
So we must adjust the density of the<br />
carbon dioxide atmosphere on Mars.<br />
You probably learned in your high<br />
school chemistry class that decreasing<br />
the temperature of a fixed amount<br />
of gas causes it to contract in volume<br />
and that decreasing the air pressure<br />
acting on it causes it to expand in volume.<br />
The equation used to calculate<br />
the volume of a gas outside of STP is:<br />
V f = V i X (T f /273) X (1013/P f )<br />
where<br />
V f is the final volume<br />
V i is the initial volume<br />
T f is the final temperature<br />
P f is the final pressure<br />
NEAR SPACE<br />
Weather Balloon, $55. Tank of Helium, $100. Photograph of the Earth from Near Space, PRICELESS.<br />
March 2006 91