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Consider 4.10 L of a gas at 365 mmHg and 20. ∘C . If the container is compressed to 2.20 L and the temperature is increased to 40. ∘C , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder. Express your answer with the appropriate units.

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Answer:

0.955 atm

Explanation:

We apply this formula derivated from the Ideal Gases Law

P₁ . V₁ / T₁ = P₂ . V₂ / T₂

We need to convert the temperature to absolute values

20°C + 273 K = 293K

40°C + 273 K = 313 K

Now we make a convertion for the pressure unit:

365 mmHg . 1 atm / 760 mmHg = 0.480 atm

We replace data:

(0.480 atm . 4.10L) / 293 K = (P₂ . 2.20 L) / 313K

[(0.480 atm . 4.10L) / 293 K] . 313 K = P₂ . 2.20 L

2.10 L.atm = P₂ . 2.20 L → P₂ = 2.10 L.atm/2.20L ⇒ 0.955 atm

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