Please note:

Starting with the report for this experiment, units obviously "filled in$"$ after calculations were completed

will be treated as "decorations" and will earn you no credit. To get full credit, you must write units at the

same time you write the numbers, and then cross out units you can cancel in the given calculation $-$ so

that the remaining unit is appropriate for the variable you calculated $($if it is not, you will know something

was done wrong$).$

A student placed some liquid nitrogen in a Styrofoam calorimeter and determined that after $64\mathrm{.}0$ seconds $5\mathrm{.}472$

$g$ of the nitrogen has vaporized $-$ just because it was exposed to ambient air at $23C.$

Calculate the rate of vaporization $($in g$/$s$)$ of liquid nitrogen exposed to ambient air at that temperature.

Rate of vaporization $=$

$\frac{g}{s}$

In the next step of the experiment, the student put $24\mathrm{.}876g$ piece of metal $($which was kept for hours at room

temperature of $23\mathrm{.}0C)$ into the calorimeter containing $239\mathrm{.}23g$ the liquid nitrogen. After a period of vigorous

boiling $($the liquid nitrogen was heated by the lab air and the metal$)$ the rate of boiling stabilized. Clearly, the heat

transfer from the metal to the liquid nitrogen was completed and the metal was "frozen" at $-196C.$ The continuous

gentle boiling $($vaporization$)$ of the liquid nitrogen was now due only to the heat transfer from the air. The student re$-$weighed

the calorimeter and found that $196\mathrm{.}0$ seconds after the metal was put into the calorimeter only $200\mathrm{.}00$ grams of

the liquid nitrogen remained. Use the provided information to calculate the heat of vaporization of liquid nitrogen in

units of $k\frac{J}{m}ol{N}_2.$ Additional data: specific heat of the metal $=0\mathrm{.}623\frac{J}{g}K$