Question #e8964
1 Answer
Explanation:
Start by taking a look at the balanced chemical equation given to you
#"C"_ 3"H"_ (8(g)) + color(blue)(4)"Cl"_ (2(g)) -> "C"_ 3"H"_ 4 "Cl"_ (4(g)) + color(purple)(4)"HCl"_ ((g))#
Notice that every mole of propane that takes part in the reaction requires
In your case,
As you can see, you have more moles of chlorine gas than you would need, since
#4.0 color(red)(cancel(color(black)("moles C"_3"H"_8))) * (color(blue)(4)color(white)(.)"moles Cl"_2)/(1color(red)(cancel(color(black)("mole C"_3"H"_8)))) = "16 moles Cl"_2#
This implies that propane acts as a limiting reagent, i.e. it is completely consumed before all the moles of chlorine gas get the chance to react.
So, you know for a fact that all the moles of propane react. You can now use the
#4.0 color(red)(cancel(color(black)("moles C"_3"H"_8))) * (color(purple)(4)color(white)(.)"moles HCl")/(1color(red)(cancel(color(black)("mole C"_3"H"_8)))) = color(darkgreen)(ul(color(black)("16 moles HCl")))#
The answer is rounded to two sig figs.