Question

Xenon hexafluoride was one of the first noble gas compounds synthesized. The solid reacts rapidly with the silicon dioxide in glass or quartz containers to form liquid XeOF4 and gaseous silicon tetrafluoride. What is the pressure in a 1.00−L container at 25° C after 8.53 g of xenon hexafluoride reacts? (Assume that silicon tetrafluoride is the only gas present and that it occupies the entire volume.)

Answer 1

0,93 atm

Step-by-step explanation:

For this we will use PV = nRT

P is what we want to find

V = 1 L

n =
`(8.53)/(223.23)` = 0,038 moles

R = 0,082
`(L atm)/(K mole)`

T = 25°C = 298,15 K

P * 1 = 0,038 *0,082 * 298,15

P = 0,93 atm