Find #K_c# for the reaction below (see details)?
#\sf{2ICl(g)\harrI_2(g)+Cl_2(g)#
A 0.0682-gram sample of #"ICl (g)"# is placed in a 625-mL reaction vessel at 628 K. When equilibrium is reached between the #"ICl (g)"# and #I_2" (g)"# formed by dissociation, 0.0383-grams of #I_2# are present.
What is #K_c# for this reaction?
Sorry if this has been asked before!
A 0.0682-gram sample of
What is
Sorry if this has been asked before!
1 Answer
Explanation:
The balanced equation of the given reversible gaseous reaction
#\sf{2ICl(g)rightleftharpoonsI_2(g)+Cl_2(g)#
Molar masses of reactant and products
Volume of reaction vessel
ICE Table
By the problem initial amount of
Amount of
The equilibrium constant
#=(x/V*x/V)/((\alpha-2x)/V)#
#=x^2/(V(\alpha-2x))#
#=(1.5xx10^-4)^2/(0.625(4.2xx10^(-4)-2*1.5xx10^-4))#
#=(2.25xx10^-8)/(0.625xx1.2xx10^-4)=3xx10^-4#