B6. At elevated temperatures,SbCl5 gas decomposes into SbCl3 gas and Cl2 gas, as shown by thefollowing equation.
SbCl5 <===> SbCl3 + Cl2
An 89.7-gram sample of SbCl5 (molecular weight 299.0) isplaced in an evacuated 15.0-liter container at 182 °C.
(1) What is the concentration in moles per liter of SbCl5 in thecontainer before any decomposition occurs?
(2) What is the pressure in atmospheres of SbCl5 in the containerbefore any decomposition occurs?
b) If the SbCl5 is 29.2 percent decomposes when equilibrium isestablished at 182 °C, calculate the value for eitherequilibrium constant, Kp or Kc, for this decomposition reaction.Indicate whether you are calculating Kp or Kc.
c) In order to produce some SbCl5, a 1.00-mole sample of SbCl3 isfirst placed in an empty 2.00-liter container maintained at atemperature different from 182 °C. At this temperature Kcequals 0.117. How many moles of Cl2 must be added to this containerto reduce the number of moles of SbCl3 to 0.700 mole atequilibrium?