Some oxygen gas takes up a volume of 2.00 liters at 0.99 atm and 273 k. its volume doubles and its temperature decreases to 137 k. what is the final pressure of the gas?
a. cannot be ddtermined
b.0.25 atm
c.0.98 atm
d.3.9 atm

The answer to your question is : letter B. 0.25 atm

Explanation:

To solve this problem we need to use the combined gas law:

    P₁V₁   =    P₂V₂

      T₁              T₂

Data

P1 = 0.99 atm  V1 = 2 l  T1 = 273K

P2 = ?               V2 = 4 l   T2 = 137K

Now, the clear P2 from the equation and we get

       P2 = P1V1T2 / T1V2

Substitution         P2 = (2 x 0.99 x 137)/(273 x 4)

       P2 = 271.26 / 1092

Result       P2 = 0.248 atm ≈ 0.25 atm

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