The stopcock connecting a 1.88 L bulb containing xenon gas at a pressure of 8.40 atm, and a 9.20 L bulb containing oxygen gas at a pressure of 3.99 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is atm?

Final pressure is 4.73 atm

Explanation:

In a mixture of gases:

Total pressure = Sum of partial pressure of each gas

Total moles = Sum of moles of each gas

We assume additives volume → 1.88L + 9.20L = 11.08L

Let's apply the Ideal Gases Law to determine the moles of Xe and O₂

P . V = n. R . T → (P. V / R . T) = n

8.40atm . 1.88L / 0.082 . 273K = n → 0.70 moles of Xe

3.99atm . 9.20L / 0.082 . 273K = n → 1.64 moles of O₂

Total moles = 0.70 moles of Xe + 1.64 moles of O₂ → 2.34 moles

P = (n . R . T) / V → (2.34 moles.  0.082L.atm/mol.K . 273 K) / 11.08L = 4.73atm

c (diamond),

sio2 (quartz)

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.