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,
#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
Plug in your values and solve for
#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")#