6 moles of #"Cl"_2# are placed in a 3L flask at 1250K. At this temperature, #"Cl"_2# begins to dissociate into #"Cl"# atoms. What is the value for #K_c# if 50.0% of the #"Cl"_2# molecules dissociate when equilibrium has been achieved?
6 moles of Cl2 are placed in a 3L flask at 1250K. At this temperature, Cl2 begins to dissociate in to Cl atoms. What is the value for Kc if 50.0% of the Cl2 molecules dissociate when equilibrium has been acheived?
6 moles of Cl2 are placed in a 3L flask at 1250K. At this temperature, Cl2 begins to dissociate in to Cl atoms. What is the value for Kc if 50.0% of the Cl2 molecules dissociate when equilibrium has been acheived?
1 Answer
Explanation:
The idea here is that you need to write a balanced chemical equation for the dissociation of chlorine gas,
So, you will have
#"Cl"_ (2(g)) rightleftharpoons color(red)(2)"Cl"_ ((g))#
Notice the every mole of chlorine gas that dissociates produces
You know that the reaction vessel initially contained
#6 color(red)(cancel(color(black)("moles Cl"_2))) * ("50 moles Cl"_2)/(100color(red)(cancel(color(black)("moles Cl"_2)))) = "3 moles Cl"_2#
You can thus say that at equilibrium, the reaction vessel will contain
#n_(Cl_2) = "6 moles" - overbrace("3 moles")^(color(blue)("50% of the initial amount")) = "3 moles Cl"_2#
and
#n_(Cl) = "0 moles" + color(red)(2) xx "3 moles" = "6 moles Cl"#
Use the volume of the vessel to calculate the concentrations of the two species
#["Cl"_2] = "3 moles"/"3 L" = "1 M"#
#["Cl"] = "6 moles"/"3 L" = "2 M"#
By definition, the *equilibrium constant for this reaction,
#K_c = (["Cl"]^color(red)(2))/(["Cl"_2])#
Plug in your values to find
#K_c = ("2 M")^color(red)(2)/"1 M" = ("4 M"^color(red)(cancel(color(black)(2))))/(1color(red)(cancel(color(black)("M")))) = "4 M"#
The equilibrium constant is usually given without added units, but keep in mind that, as you can see in this example, that is not always the case
#K_c = color(green)(|bar(ul(color(white)(a/a)color(black)(4)color(white)(a/a)|)))#
The answer is rounded to one sig fig, the number of sig figs you have for the number of moles of chlorine gas added to the reaction vessel and for the volume of the vessel.