Question #3ccd4
1 Answer
Explanation:
Your tool of choice here is the ideal gas law equation, which looks like this
#color(blue)(ul(color(black)(PV = nRT)))#
Here
#P# is the pressure of the gas#V# is the volume it occupies#n# is the number of moles of gas present in the sample#R# is the universal gas constant, equal to#0.0821("atm L")/("mol K")# #T# is the absolute temperature of the gas
Now, the problem wants you to find the density of nitrogen dioxide in a volume of
#28^@"C" = 28^@"C" + 273.15 = "301.15 K"#
and a pressure of
As you know, the density of a substance,
#color(blue)(rho = m/V)#
Now, notice that the ideal gas law equation uses the number of moles of gas,
#n = m/M_M#
Plug this into the ideal gas law equation to get
#PV = m/M_M * RT#
All you have to do now is to rearrange this equation in order to find an expression for the density of the gas.
#P = color(blue)(m)/(M_M * color(blue)(V)) * RT#
#P * M_M = color(blue)(m)/color(blue)(V) * RT#
This means that you have
#P * M_M = color(blue)(rho) * RT#
which gets you
#color(blue)(rho) = (P * M_M)/(RT)#
Finally, plug in your values to find
#rho = (0.85 color(red)(cancel(color(black)("atm"))) * "46.0 g" color(red)(cancel(color(black)("mol"^(-1)))))/(0.0821(color(red)(cancel(color(black)("atm"))) * "L")/(color(red)(cancel(color(black)("mol"))) * color(red)(cancel(color(black)("K")))) * 301.15 color(red)(cancel(color(black)("K")))) = color(darkgreen)(ul(color(black)("1.6 g L"^(-1))))#
The answer is rounded to two sig figs.
Notice that you didn't need to know the volume of the gas in order to be able to find its density.