What is the celsius temperature of 100.0 g of chlorine gas in a 40.0-L container at 800 mm Hg?

Feb 22, 2017

This question is ill-proposed..........I get approx.. $136$ ""^@C

Explanation:

$1 \cdot a t m$ will support a column of mercury that is $\text{760 mm}$ high. Often we can use the length of a mercury column to measure a reduced pressure, using the relationship, $1 \cdot a t m \equiv \text{760 mm Hg}$.

If we try to use a column of mercury that is higher than $\text{760 mm}$, we risk getting mercury all over the lab, where it will inhabit every nook and every cranny.

We assume a pressure of "800 mm Hg"/("760 mm Hg"*atm^-1)=1.053*atm.

We use the Ideal Gas equation, $T = \frac{P V}{n R}$

$\frac{1.053 \cdot \cancel{a t m} \times 40.0 \cdot \cancel{L}}{\frac{100.0 \cdot \cancel{g}}{70.9 \cdot \cancel{g} \cdot \cancel{m o {l}^{-} 1}} \times 0.0821 \cdot \cancel{L} \cdot \cancel{a t m} \cdot {K}^{-} 1 \cdot \cancel{m o {l}^{-} 1}} = 409.9 \cdot K$

What is this temperature in $\text{degrees Celsius}$?