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Korolek [52]
3 years ago
14

Consider 4.60 L of a gas at 365 mmHg and 20 C . If the container is compressed to 2.60 L and the temperature is increased to 36

C , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder.
Chemistry
1 answer:
BaLLatris [955]3 years ago
6 0

Explanation:

The given data is as follows.

       V_{1} = 4.60 L,        P_{1} = 365 mm Hg

       V_{2} = 2.60 L,       P_{2} = ?

       T_{1} = (20 + 273) K = 293 K,      T_{2} = (36 + 273) K = 309 K

Since, number of moles of gas are equal so, according to ideal gas equation:

          \frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}

          \frac{365 mm Hg \times 4.60 L}{293 K} = \frac{P_{2} \times 2.60 L}{309 K}

          P_{2} = 681.03 mm Hg

Thus, we can conclude that new pressure P_{2} is 681.03 mm Hg.

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