A 9.95*mol quantity of ideal gas is placed in a container of 208*L volume at 1.26*atm pressure. What is the temperature of the gas?

Apr 26, 2017

We can assume ideality, and find $T \cong 320 \cdot K$

Explanation:

$T = \frac{P V}{n R} = \frac{1.26 \cdot \cancel{a t m} \times 208 \cdot \cancel{L}}{9.95 \cdot \cancel{m o l} \times 0.0821 \cdot \cancel{L \cdot a t m} \cdot {K}^{-} 1 \cdot \cancel{m o {l}^{-} 1}}$

At least this is dimensionally consistent. We wanted an answer in $K$, we got an answer in $\frac{1}{{K}^{-} 1} = \frac{1}{\frac{1}{K}} = K$ as required............

So two questions:

From where did I get the expression $T = \frac{P V}{n R}$?

If we had measured $\text{ammonia gas}$ or $\text{hydrogen chloride}$ would our assumption of ideality be justified?