A closed container contains 0.0300 mol of Ar (g) and a sample of the solid, ammonium bromide NH4Br. Assume that the volumes of solids are negligible compared to the volume of the container. The pressure of the Ar is measured at 31 degrees Celsius and is found to be 0.153 atm. The container is then heated to 331 degrees Celsius and all of the ammonium bromide decomposes according to the reaction:
NH4Br(s)-->NH3(g)+HBr(g)
The Ar is not involved in the reaction and is still present.
The final pressure in the container after complete decomposition of thr NH4Br is 1.31 atm.
Assuming ideal gas behavior, answer the following questions.
a) What is the volume of the container, in liters?
b) How many moles of gas are present after the reaction has come to completion?
c) What is the mol fraction of Ar after the reaction has come to completion?
d) What is the partial pressure of HBr in the container, at 331 degrees Celsius, when the reacion is complete?