The following shows 1.00L bulbs connected by valves. Each bulb contains neon gas with amounts proportional to the number of atoms pictorially reprsented in each chamber. All three bulbs are maintained at the same temperature. Unless stated otherwise, assume that hte valves connecting champers are closed and seal the gases in their respective chambers. Assume also that the volume between chambers is negligible. B C If the pressure in bulb A is 2.00atm, what is the pressure in bulb C? (Answer in atm, no units.)

A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 tor. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)

A typical barometric pressure in Redding. California, is about 750 mm Hg. Calculate this pressure in atm and kPa.

You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.