What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2°C when it occupies a volume of 5.00 L?

Jul 23, 2017

$31.92$

Explanation:

To solve this problem we will use the ideal gas law equation:

$P V = n R T$

To find pressure we divided both sides by $V$

$\frac{P \cancel{V}}{\cancel{V}} = \frac{n R T}{V}$

$P = \frac{n R T}{V}$

First we need to convert the temperature to K so we add $212$

46.2°C +212K=258.2K

Now we also need to find the number of moles first we find the molar mass of $C {O}_{2}$, which is 44. We take our $.44$ and divided by $44$.

$\left(\text{gram sample of carbon dioxide")/("molar mass of } C {O}_{2}\right)$

(.44 " grams")/(44 " Molar mass")=.01 " moles"

Now we have:

$n = .01$

$R = 0.0806$ This is the universal gas constant

$T = 258.2 K$

$V = 5.00 L$

Let's plug it in:

$P = \frac{.01 \text{moles} \left(0.0806 \frac{L \times a t m}{m o l \times K} \left(258.2 K\right)\right)}{5.00 L}$

$P = .042 \text{ atm}$

To find the torr you multiply:

$.042 \times 760 = 31.92$