If the pressure on a gas decreases from 1480 mm Hg at 478 K to 555 mm Hg, what is the final temperature? V​1​ = P​1​ = T​1​ =
V​2​ =
Law:
P​2​ =
T​2​ =

179 K

Explanation:

From the question given above, the following data were:

Initial pressure (P₁) = 1480 mm Hg

Initial temperature (T₁) = 478 K

Final pressure (P₂) = 555 mm Hg

Final temperature (T₂) =?

The final temperature of the gas can be obtained as follow:

P₁/T₁ = P₂/T₂

1480 / 478 = 555 / T₂

Cross multiply

1480 × T₂ = 478 × 555

1480 × T₂ = 265290

Divide both side by 1480

T₂ = 265290 / 1480

T₂ ≈ 179 K

Therefore, the final temperature of the gas is 179 K

the answer for sodium is 0.186

the answer for rubidium is 0.251

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

if you need further assistance, let me know: )

~ trueboss72