I calculated the partial pressure to be 16.1 - and it was wrong?
Consider the following equilibrium reaction at #256^circC# .
#SbCl_(5"(g)")⇌SbCl_("3(g)") + Cl_(2"(g)")#
If the equilibrium constant in terms of concentrations (#K_c# ) is #3.7 xx 10^-2# , calculate the equilibrium constant in terms of partial pressures (#K_p# ).
Consider the following equilibrium reaction at
If the equilibrium constant in terms of concentrations (
1 Answer
Feb 20, 2018
Explanation:
#K_c# = equilibrium constant in terms of pressure#R# = gas constant (#8.31"J"# #"K"^-1# #"mol"^-1# )#T# = absolute temperature (#K# )#Deltan="Number of moles of gaseous products"-"Number of moles of gaseous reactants"#