a rigid, closed container contains 0.0100mol He(g) and a sample of a solid, ammonium bromide, NH4Br. Assume that the volume of the solids are negligible compared to the volume of the container. The pressure of the He is measured at 29C and is found to be 0.0918 atm. the container is heated to 329C and all of the ammonium bromide decomposes according to the reaction: NH4Br(s) --->NH3(s) + HBr(s). The He is not involved in this reaction and is still present. the final pressure in the container after decompostion of the NH4Br is 2.74 atm. Assuming ideal gas behavior, answer the following question:
a) what is the volume of the container, in liters?
b)What is the partial pressure of HBr in the container, at 329C, when the reaction is complete?