At a certain temperature, #"PCl"_5(g)# decomposes. What are the concentrations of #"PCl"_5# and #"PCl"_3# in a #"3.70-L"# container that begins with #"0.287 mols"# #"PCl"_5(g)# that dissociates? #K_c = 1.80# at this temperature.
1 Answer
I'll let you decide which is which, by reading the answer down below. ;)
Construct an ICE table and mass action expression in terms of concentration:
#"PCl"_5(g) rightleftharpoons "PCl"_3(g) + "Cl"_2(g)#
#"I"" "0.287/3.70" "" "" "0" "" "" "0#
#"C"" "-x" "" "" "+x" "" "+x#
#"E"" "0.287/3.70 - x" "x" "" "" "x#
And thus,
#K_c = x^2/(0.287/3.70 - x)#
#0.287/3.70K_c - K_cx = x^2#
#=> x^2 + K_cx - 0.287/3.70K_c#
#= x^2 + 1.80x - 0.1396 = 0#
Solve to obtain a physical value of
#[PCl_5] = 0.287/3.70 - 0.0745 = ul"0.00308 M"#
#[PCl_3] = ul"0.0745 M"#
Why would the small