The stopcock connecting a 1.83 l bulb containing helium gas at a pressure of 2.60 atm, and a 6.48 l bulb containing xenon gas at a pressure of 3.56 atm, is opened and the gases are allowed to mix. assuming that the temperature remains constant, what is the final pressure in the system is atm?

P(final) = 6.16 atm

Explanation:

Solution:

According to the Dalton's law of partial pressure,

"The total pressure exerted by the mixture of gases is the sum of partial pressure of the individual gases"

P(total) = P₁ + P₂ + P₃ +Pₙ

Given data:

Pressure of helium gas = 2.60 atm

Volume of 1st bulb = 1.83 L

Pressure of xenon gas = 3.56 atm

Volume of 2nd bulb = 6.48 L

Final pressure after mixing of gases=?

Formula:

P(final) = P(helium) + P(xenon)

P(final) = 2.60 atm  + 3.56 atm

P(final) = 6.16 atm

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

im pretty sure its b