Here's what you could do here.
The tricky thing to remember about gases is that their volume depends on the conditions for pressure and temperature.
In other words, the mass of carbon monoxide that occupies
Since you didn't provide any information about the temperature and the pressure at which the sample is kept, I'll assume that you're working at STP conditions.
Now, STP conditions are defined as a pressure of
#"1 mole of an ideal gas" color(white)(aaaa) stackrel(color(white)(acolor(blue)("at STP")aaa))(->) color(white)(underbrace(color(black)("22.7 L"))_ (color(red)("molar volume of a gas at STP"))#
So, use the molar volume of a gas at STP to calculate the number of moles of carbon monoxide present in your sample
#134 color(red)(cancel(color(black)("L"))) * "1 mole CO"/(22.7color(red)(cancel(color(black)("L")))) = "5.903 moles CO"#
To convert this to grams, use the molar mass of carbon monoxide
#5.903 color(red)(cancel(color(black)("moles CO"))) * "28.01 g"/(1color(red)(cancel(color(black)("mole CO")))) = color(darkgreen)(ul(color(black)("165 g")))#
The answer is rounded to three sig figs, the number of sig figs you have for the volume of the sample.