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?

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Answer 1 · 2017-07-23T21:14:00

$31.92$

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

$PV=nRT$

To find pressure we divided both sides by $V$

$(PcancelV)/cancelV=(nRT)/V$

$P=(nRT)/V$

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 $CO_2$ , which is 44. We take our $.44$ and divided by $44$ .

$("gram sample of carbon dioxide")/("molar mass of " CO_2)$

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

Now we have:

$n=.01$

$R=0.0806$ This is the universal gas constant

$T=258.2K$

$V=5.00L$

Let's plug it in:

$P=(.01"moles"(0.0806(Lxxatm)/(molxxK)(258.2K)))/(5.00L)$

$P=.042 " atm"$

To find the torr you multiply:

$.042xx760=31.92$