Question #3c541
1 Answer
Here's what I got.
Explanation:
Your starting point here will be the balanced chemical equations for the combustion of these two gases, methane,
#"C"_2"H"_text(4(g]) + color(red)(3)"O"_text(2(g]) -> 2"CO"_text(2(g]) + 2"H"_2"O"_text((g])#
#"CH"_text(4(g]) + color(blue)(2)"O"_text(2(g]) -> "CO"_text(2(g]) + 2"H"_2"O"_text((g])#
Take a look at the mole ratios that exist between the two gases and oxygen. You will see that
- every mole of ethylene will require
#color(blue)(3)# moles of oxygen gas- every mole of methane will require
#color(red)(2)# moles of oxygen gas
Now, let's assume that
#x + y = "0.3 moles" " " " "color(purple)((1))#
Now, since no mention of pressure and temperature was made, I"ll assume that you're working at STP, Standard Temperature and Pressure.
At STP conditions, which are defined as a pressure of
Use the molar volume of a gas to find how many moles of oxygen were needed for the combustion of the mixture
#15.68 color(red)(cancel(color(black)("L"))) * "1 mole O"_2/(22.7color(red)(cancel(color(black)("L")))) = "0.69075 moles O"_2#
So, if
#x color(red)(cancel(color(black)("moles C"_2"H"_4))) * (color(red)(3)" moles O"_2)/(1color(red)(cancel(color(black)("mole C"_2"H"_4)))) = color(red)(3)x" moles O"_2#
Likewise, if
#y color(red)(cancel(color(black)("moles C"_2"H"_4))) * (color(blue)(2)" moles O"_2)/(1color(red)(cancel(color(black)("mole C"_2"H"_4)))) = color(blue)(2)y" moles O"_2#
This means that you have
#color(red)(3)x + color(blue)(2)y = "0.69075 moles O"_2" " " "color(purple)((2))#
Since you need to find the mass of methane present in the mixture, solve these two equations for
#x = 0.3 - y#
Plug this into equation
#3 * (0.3 - y) + 2y = 0.69075#
#0.9 -3y + 2y = 0.69075#
#y = 0.20925#
So, your initial mixture contained
#0.20925 color(red)(cancel(color(black)("moles CH"_4))) * "16.0425 g"/(1color(red)(cancel(color(black)("mole CH"_4)))) = "3.357 g"#
I'll leave the answer rounded to two sig figs
#m_(CH_4) = color(green)("3.4 g")#
SIDE NOTE Many sources still use the old definition of STP, at which pressure is equal to
Under these conditions for pressure and temperature, one mole of any ideal gas occupies