# A #89.9# g sample of dinitrogen monoxide is confined in a #3.65#-L vessel. What is the pressure (in atm) at #110# degrees Celsius?

##### 1 Answer

#### Explanation:

All you have to do here is use *nitrous oxide*'s molar mass to determine how many moles you have in that sample, then use the ideal gas law equation to find its pressure.

Nitrous oxide, **one mole** of nitrous oxide will have a mass of

#89.9color(red)(cancel(color(black)("g"))) * ("1 mole N"_2"O")/(44.013color(red)(cancel(color(black)("g")))) = "2.043 moles N"_2"O"#

Now, the ideal gas law equation looks like this

#color(blue)(PV = nRT)" "# , where

*universal gas constant*, equal to

Plug in your values and solve for *degrees Celsius* to *Kelvin*

#PV = nRT implies P = (nRT)/V#

#P = (2.043color(red)(cancel(color(black)("moles"))) * 0.082("atm" * color(red)(cancel(color(black)("L"))))/("mol" * color(red)(cancel(color(black)("K")))) * (273.15 + 110)color(red)(cancel(color(black)("K"))))/(3.65color(red)(cancel(color(black)("L"))))#

#P = "17.59 atm"#

Rounded to two sig figs, the number of sig figs you have for the temperature of the gas, the answer will be

#P = color(green)("18 atm")#