Suppose 2.4 moles of xenon difluoride vapor at 550.00 $\circ$ C and 16.2 atm in a 10.0 L tank decompose completely to form xenon gas and fluorine gas,which are then allowed to cool to 25.00 $\circ$ C.What is the final pressure? XeF₂(g)$\to$ Xe(g)+ F₂(g)

Question

Quizplus · Accepted Answer

The decomposition of XeF2 results in the formation of 1 mole of Xe and 1 mole of F2 for each mole of XeF2, doubling the number of moles of gas. Using the ideal gas law and considering the change in temperature and volume, the final pressure is calculated to be 11.7 atm.

Suppose 24 Moles of Xenon Difluoride Vapor at 550 ∘\circ∘ C and 16

Suppose 24 Moles of Xenon Difluoride Vapor at 550 $\circ$ C and 16