# At what temperature will 14.0 g of H_2 occupy a volume of 15.5L at a pressure of 204 kPa?

Jan 19, 2017

$T = \frac{P V}{n R} \cong 50 \cdot K$

#### Explanation:

Of course, we need to find the appropriate gas constant.

This site gives me $R = 8.314 \cdot L \cdot k P a \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$.

Given this, we plug in the numbers:

$T = \frac{204 \cdot k P a \times 15.5 \cdot L}{\frac{14.0 \cdot g}{2.016 \cdot g \cdot m o {l}^{-} 1} \times 8.314 \cdot L \cdot k P a \cdot {K}^{-} 1 \cdot m o {l}^{-} 1}$

We should get an answer in $\frac{1}{K} ^ - 1 = \frac{1}{\frac{1}{K}} = K$ as required for an $\text{absolute temperature}$.

The temperature is so low because there is a large molar quantity of dihydrogen. At this temperature we would anticipate some deviation from ideality. We are in no position to assess this.