Mount Everest rises to a height of 8,850 m above sea level. At a base camp on the mountain the atmospheric pressure is measured to be 314.0 mm Hg. At what temperature (in °C) will water boil at base camp ? The vapor pressure of water at 373 K is 760.0 mm Hg. (ΔH°vap for H2O = 40.7 kJ/mol and R = 8.314 J/mol K).
a. 344°C.
b. 70.8°C .
c. 2.91E-3°C .
d. 79.8°C.
e. 57.8°C.

Water will boil at .

Explanation:

According to clausius-clapeyron equation for liquid-vapor equilibrium:

where, and are vapor pressures of liquid at (in kelvin) and (in kelvin) temperatures respectively.

Here, = 760.0 mm Hg, = 373 K, = 314.0 mm Hg

Plug-in all the given values in the above equation:

                       or,

So,

Hence, at base camp, water will boil at

is has three carbons, so the answer is propylamine.

meth-

eth-

prop-

but-

pent-

hex-

hept-

oct-

non-

explanation:

- both b and d.

-since b and d are the closest coastlines then that makes it the most affected.

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