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.

am i too late?

explanation: