At elevated temperatures SbCl5 gas decomposes into SbCl3 gas and Cl2 gas, as shown by the following equation:
SbCl5<=> SbCl3 + Cl2
A) An 89.7 gram sample of SbCl5 (molecular weight 299.0) is placed in an evacuated 15.0 liter at 182 celsius
I) What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs?
II) What is the preassure in atmospheres of SbCl5 in the container before any decomposition occurs? PV=nRT
B) If the SbCl5 is 29.2% decomposes when equilibrium is established at 182 celsius, calculate the value for either equilibrium constant, Kc, for this decomposition reaction.
C) In order to produce some SbCl5 a 1.00 mole sample of SbCl3 is first placed in an empty 2.00 liter container maintained at a temperature different from 182 celsius. At this temperature Kc equals 0.117. How many moles of Cl2 must be added to this container to reduce the number of moles of SbCl3 to 0.700 moles at equilibrium?