A gas has a volume of 14.5 L at 22.9 Celsius and 3.4 atm. what will the new volume be at 44.5 Celsius and 778 torr?

51.8 L is the new volume

Explanation:

In the two situations we have this relationship:

P ₁ . V₁ / T₁ = P₂ . V₂ / T₂

Let's convert the temperature to absolute values

T°K = T°C + 273

22.9°C + 273 = 295.9 K

44.5°C + 273 = 317.5 K

Let's convert now, the Torr to atm.

778 Torr . 1 atm / 760 Torr = 1.02 atm

Now we can replace:

3.4 atm . 14.5L / 295.9K = 1.02 atm . V₂ / 317K

(3.4 atm . 14.5L / 295.9K) . 317 K = 1.02 atm . V₂

( (3.4 atm . 14.5L / 295.9K) . 317 K ) / 1.02 atm = V₂ → 51.8 L

P ₁ . V₁ / T₁ = P₂ . V₂ / T₂ is derived from the Ideal Gases Law equation, and it is fulfilled when the moles of a gas, remains constant after the change of T°, pressure and volume.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

lol idk man i guess u gotta ask bill nye the science guy