If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant, what final pressure would result if the original pressure was 750.0 mm Hg? Round to the nearest tenth. Don't forget the units.

(P1/T1) = (P2/T2)

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To find the final pressure of the gas when it is cooled with constant volume, we can use the relationship known as Charles' Law, which states that for a given amount of gas at constant pressure, the volume of the gas is directly proportional to its absolute temperature.

Given:
Initial temperature (T₁) = 323.0 K
Final temperature (T₂) = 273.15 K
Initial pressure (P₁) = 750.0 mm Hg

Since the volume is kept constant, we can assume the volume (V₁) = V₂.
According to Charles' Law, we have:

(V₁/T₁) = (V₂/T₂)

Solving the equation for V₂:
V₂ = (V₁ * T₂) / T₁

Since the volume is constant, V₁ = V₂, so we can rewrite the equation as:

V₁ = (V₁ * T₂) / T₁

Now, let's substitute the given values:

750.0 mm Hg = (V₁ * 273.15 K) / 323.0 K

To find V₁, we can cross multiply:

750.0 mm Hg * 323.0 K = V₁ * 273.15 K

V₁ = (750.0 mm Hg * 323.0 K) / 273.15 K

V₁ ≈ 888.9 mm Hg (rounded to the nearest tenth)

Therefore, the final pressure would be approximately 888.9 mm Hg when the gas is cooled to 273.15 K with constant volume.